Final laboratory test

Water analysis

1. The acidity of the water is due to:
   1. hydroxides from water;
   2. all minerals dissolved in water;
   3. free carbon dioxide, mineral acids and salts of strong acids with weak bases;
   4. only insoluble salts;
2. Water softening is based on passing the water on:
   1. fractionation columns;
   2. cooling columns;
   3. distillation columns;
   4. ion exchange columns;
3. At the titration of water samples:
   1. the burette reads only at the start of titration process;
   2. the burette reads before the start of titration and at the end of titration;
   3. is added sulphuric acid in the samples;
   4. does not need to be read the burette;
4. The experiment for the analysis of drinking water:
   1. was intended water purification;
   2. was aimed, at the wareness of the risks to which we expose drinking tap water;
   3. was aimed at the determination of alkalinity;
   4. was aimed at determination of the cations from water
5. In order to determine the acidity of decationized water, the samples:
   1. are titrated with natrium hydroxide in presence of phenolphthalein;
   2. are titrated with hydrochloric acid in presence of methyl orange;
   3. none of the answers are correct;
   4. are titrated with sulphuric acid in presence of ERIO T;

Final laboratory test

Water analysis

1. When is determining temporary hardness titration of water samples is made:
   1. with sodium hydroxide in the presence of phenolphthalein until the appearance of pink color;
   2. with clorhidric acid in the presence of methyl orange until the appearance of orange color;
   3. with sulphuric acid in the presence of methyl orange until the appearance of brown color;
   4. with potasium hydroxide;
2. At the determination of total hardness in water sample:
   1. ia added oxalic acid and then the sample is titrated with permanganate solution;
   2. is formed a blue color complex after titration;
   3. just add ERIO T and titrate;
   4. is directly titrated with EDTA solution;
3. The acidity of the water is due to:
   1. hydroxides from water;
   2. all minerals dissolved in water;
   3. free carbon dioxide, mineral acids and salts of strong acids with weak bases;
   4. only insoluble salts;
4. The experiment for the analysis of drinking water:
   1. was intended water purification;
   2. was aimed, at the wareness of the risks to which we expose drinking tap water;
   3. was aimed at the determination of alkalinity;
   4. was aimed at determination of the cations from water
5. In order to determine the acidity of decationized water, the samples:
   1. are titrated with natrium hydroxide in presence of phenolphthalein;
   2. none of the answers are correct;
   3. are titrated with sulphuric acid in presence of ERIO T;
   4. are titrated with hydrochloric acid in presence of methyl orange;

Final laboratory test

Water analysis

1. In order to determine the acidity of decationized water, the samples:
   1. none of the answers are correct;
   2. are titrated with natrium hydroxide in presence of phenolphthalein;
   3. are titrated with hydrochloric acid in presence of methyl orange;
   4. are titrated with sulphuric acid in presence of ERIO T;
2. At the determination of total hardness in water sample:
   1. ia added oxalic acid and then the sample is titrated with permanganate solution;
   2. is formed a blue color complex after titration;
   3. just add ERIO T and titrate;
   4. is directly titrated with EDTA solution;
3. When is determining temporary hardness titration of water samples is made:
   1. with potasium hydroxide;
   2. with sodium hydroxide in the presence of phenolphthalein until the appearance of pink color;
   3. with sulphuric acid in the presence of methyl orange until the appearance of brown color;
   4. with clorhidric acid in the presence of methyl orange until the appearance of orange color;
4. The experiment for the analysis of drinking water:
   1. was aimed at the determination of alkalinity;
   2. was intended water purification;
   3. was aimed at determination of the cations from water
   4. was aimed, at the wareness of the risks to which we expose drinking tap water;
5. Water softening is based on passing the water on:
   1. fractionation columns;
   2. ion exchange columns;
   3. distillation columns;
   4. cooling columns;

Final laboratory test

Water analysis

1. At the titration of water samples:
   1. does not need to be read the burette;
   2. is added sulphuric acid in the samples;
   3. the burette reads before the start of titration and at the end of titration;
   4. the burette reads only at the start of titration process;
2. In order to determine the acidity of decationized water, the samples:
   1. none of the answers are correct;
   2. are titrated with natrium hydroxide in presence of phenolphthalein;
   3. are titrated with hydrochloric acid in presence of methyl orange;
   4. are titrated with sulphuric acid in presence of ERIO T;
3. The acidity of the water is due to:
   1. free carbon dioxide, mineral acids and salts of strong acids with weak bases;
   2. only insoluble salts;
   3. all minerals dissolved in water;
   4. hydroxides from water;
4. At the determination of total hardness in water sample:
   1. is directly titrated with EDTA solution;
   2. just add ERIO T and titrate;
   3. is formed a blue color complex after titration;
   4. ia added oxalic acid and then the sample is titrated with permanganate solution;
5. When is determining temporary hardness titration of water samples is made:
   1. with sodium hydroxide in the presence of phenolphthalein until the appearance of pink color;
   2. with potasium hydroxide;
   3. with clorhidric acid in the presence of methyl orange until the appearance of orange color;
   4. with sulphuric acid in the presence of methyl orange until the appearance of brown color;

Final laboratory test

Water analysis

1. At the titration of water samples:
   1. the burette reads only at the start of titration process;
   2. is added sulphuric acid in the samples;
   3. does not need to be read the burette;
   4. the burette reads before the start of titration and at the end of titration;
2. In order to determine the acidity of decationized water, the samples:
   1. are titrated with natrium hydroxide in presence of phenolphthalein;
   2. none of the answers are correct;
   3. are titrated with sulphuric acid in presence of ERIO T;
   4. are titrated with hydrochloric acid in presence of methyl orange;
3. Water softening is based on passing the water on:
   1. ion exchange columns;
   2. distillation columns;
   3. cooling columns;
   4. fractionation columns;
4. When is determining temporary hardness titration of water samples is made:
   1. with sodium hydroxide in the presence of phenolphthalein until the appearance of pink color;
   2. with clorhidric acid in the presence of methyl orange until the appearance of orange color;
   3. with potasium hydroxide;
   4. with sulphuric acid in the presence of methyl orange until the appearance of brown color;
5. At the determination of total hardness in water sample:
   1. is formed a blue color complex after titration;
   2. ia added oxalic acid and then the sample is titrated with permanganate solution;
   3. just add ERIO T and titrate;
   4. is directly titrated with EDTA solution;

Final laboratory test

Solution concentration

1. Titration is a laboratory operation, which is performed in the presence of:
   1. a pH indicator that changes color depending on the pH of the solution;
   2. a salt;
   3. sulphuric acid;
   4. natrium hydroxide;
2. Changing the color of pH indicator shows that:
   1. equivalent point;
   2. titration process should be continued;
   3. resumption of titration;
   4. does not have any effect on the process of titration;
3. In the calculation, of oxalic acid factor solution:
   1. its actual titer reads from the working procedure of laboratory work;
   2. its actual titer reads before and after the titration from the burette;
   3. it is not necessary to read the real titer;
   4. its actual titer reads from the reagent bottle label;
4. Acid-base titration of the three samples of sulfuric acid with sodium hydroxide, is carried out until the appearance of:
   1. none of the answers are correct;
   2. the orange color;
   3. the yellow color;
   4. the dark-brown color;
5. Reactions between acids and bases:
   1. have as a consequence the dissolution of a salt;
   2. have as a consequence the formation of a quantity of water;
   3. are all exothermic;
   4. are always fast, taking place almost instantaneously;

Final laboratory test

Solution concentration

1. Changing the color of pH indicator shows that:
   1. equivalent point;
   2. resumption of titration;
   3. titration process should be continued;
   4. does not have any effect on the process of titration;
2. Acid-base titration of the three samples of sulfuric acid with sodium hydroxide, is carried out until the appearance of:
   1. the yellow color;
   2. none of the answers are correct;
   3. the dark-brown color;
   4. the orange color;
3. At the redox titration with potassium permanganate solution, the samples were heated for:
   1. has no effect;
   2. to stop the chemical reaction that occurs in the titration;
   3. trigger and speed up the reaction;
   4. decrease the reaction rate;
4. The oxidation is the process of:
   1. donation of electrons, and increasing the oxidation number;
   2. donation of electrons, and decreasing the oxidation number;
   3. acceptance of electrons, and increasing the oxidation number;
   4. acceptance of electrons, and decreasing the oxidation number;
5. Reactions between acids and bases:
   1. are always fast, taking place almost instantaneously;
   2. have as a consequence the dissolution of a salt;
   3. have as a consequence the formation of a quantity of water;
   4. are all exothermic;

Final laboratory test

Solution concentration

1. Reactions between acids and bases:
   1. are all exothermic;
   2. have as a consequence the formation of a quantity of water;
   3. have as a consequence the dissolution of a salt;
   4. are always fast, taking place almost instantaneously;
2. The oxidation is the process of:
   1. acceptance of electrons, and decreasing the oxidation number;
   2. donation of electrons, and increasing the oxidation number;
   3. acceptance of electrons, and increasing the oxidation number;
   4. donation of electrons, and decreasing the oxidation number;
3. Changing the color of pH indicator shows that:
   1. equivalent point;
   2. titration process should be continued;
   3. does not have any effect on the process of titration;
   4. resumption of titration;
4. In the calculation, of oxalic acid factor solution:
   1. its actual titer reads from the working procedure of laboratory work;
   2. its actual titer reads before and after the titration from the burette;
   3. its actual titer reads from the reagent bottle label;
   4. it is not necessary to read the real titer;
5. Acid-base titration of the three samples of sulfuric acid with sodium hydroxide, is carried out until the appearance of:
   1. the dark-brown color;
   2. none of the answers are correct;
   3. the yellow color;
   4. the orange color;

Final laboratory test

Solution concentration

1. Reactions between acids and bases:
   1. are always fast, taking place almost instantaneously;
   2. have as a consequence the dissolution of a salt;
   3. have as a consequence the formation of a quantity of water;
   4. are all exothermic;
2. At the redox titration with potassium permanganate solution, the samples were heated for:
   1. trigger and speed up the reaction;
   2. to stop the chemical reaction that occurs in the titration;
   3. decrease the reaction rate;
   4. has no effect;
3. The oxidation is the process of:
   1. acceptance of electrons, and increasing the oxidation number;
   2. acceptance of electrons, and decreasing the oxidation number;
   3. donation of electrons, and decreasing the oxidation number;
   4. donation of electrons, and increasing the oxidation number;
4. Changing the color of pH indicator shows that:
   1. titration process should be continued;
   2. resumption of titration;
   3. does not have any effect on the process of titration;
   4. equivalent point;
5. Acid-base titration of the three samples of sulfuric acid with sodium hydroxide, is carried out until the appearance of:
   1. the yellow color;
   2. the orange color;
   3. none of the answers are correct;
   4. the dark-brown color;

Final laboratory test

Solution concentration

1. The oxidation is the process of:
   1. donation of electrons, and decreasing the oxidation number;
   2. acceptance of electrons, and increasing the oxidation number;
   3. donation of electrons, and increasing the oxidation number;
   4. acceptance of electrons, and decreasing the oxidation number;
2. Changing the color of pH indicator shows that:
   1. resumption of titration;
   2. does not have any effect on the process of titration;
   3. titration process should be continued;
   4. equivalent point;
3. In the calculation, of oxalic acid factor solution:
   1. it is not necessary to read the real titer;
   2. its actual titer reads from the working procedure of laboratory work;
   3. its actual titer reads from the reagent bottle label;
   4. its actual titer reads before and after the titration from the burette;
4. Reactions between acids and bases:
   1. have as a consequence the formation of a quantity of water;
   2. are all exothermic;
   3. are always fast, taking place almost instantaneously;
   4. have as a consequence the dissolution of a salt;
5. At the redox titration with potassium permanganate solution, the samples were heated for:
   1. decrease the reaction rate;
   2. has no effect;
   3. to stop the chemical reaction that occurs in the titration;
   4. trigger and speed up the reaction;

Final laboratory test

Metal corrosion

1. The corrosion rate is:
   1. variation of the sample mass per unit area, per unit time;
   2. sample size variation per unit time;
   3. variation of the sample mass, per unit time;
   4. variation of the sample mass per unit area;
2. When calculating the corrosion rate the surface is expressed in:
   1. cm²;
   2. m³;;
   3. m²;
   4. dm²;
3. In the gravimetric method, aluminum plate:
   1. is not necessary, weighing the aluminum sample;
   2. is weight only after immersion;
   3. is degreased in sodium hydroxide solution;
   4. is weighed before and after immersing it in NaOH;
4. In corrosion processes studied gas is released:
   1. which is a volume that depends on the amount of metal corroded;
   2. which is a volume that does not depend on the sample surface;
   3. only the corrosion of aluminum;
   4. only the corrosion of zinc;
5. At the volumetric method:
   1. degrease the sample in sulfuric acid solution;
   2. the sample size of zinc are measured, and then weighed the sample;
   3. weigh the zinc before and after the process takes place;
   4. is not required, weighing the sample of zinc;

Final laboratory test

Metal corrosion

1. At the volumetric method:
   1. degrease the sample in sulfuric acid solution;
   2. weigh the zinc before and after the process takes place;
   3. is not required, weighing the sample of zinc;
   4. the sample size of zinc are measured, and then weighed the sample;
2. The corrosion rate is:
   1. variation of the sample mass per unit area;
   2. sample size variation per unit time;
   3. variation of the sample mass, per unit time;
   4. variation of the sample mass per unit area, per unit time;
3. When calculating the corrosion rate the surface is expressed in:
   1. m³;;
   2. cm²;
   3. m²;
   4. dm²;
4. In corrosion processes studied gas is released:
   1. which is a volume that depends on the amount of metal corroded;
   2. only the corrosion of aluminum;
   3. only the corrosion of zinc;
   4. which is a volume that does not depend on the sample surface;
5. Resistance grouping of the two samples studied in the laboratory is based on:
   1. their size, and time that are subject to chemical agents;
   2. the surface of the samples;
   3. their mass;
   4. the value of penetration index;

Final laboratory test

Metal corrosion

1. Corrosion of metals is:
   1. a beneficial process that shows the stability of metals;
   2. the protection in time to chemical agents;
   3. the destruction of metals under the action of external factors;
   4. the cleaning of metals;
2. When calculating the corrosion rate the surface is expressed in:
   1. m²;
   2. cm²;
   3. m³;;
   4. dm²;
3. Resistance grouping of the two samples studied in the laboratory is based on:
   1. their size, and time that are subject to chemical agents;
   2. their mass;
   3. the value of penetration index;
   4. the surface of the samples;
4. The corrosion rate is:
   1. variation of the sample mass per unit area, per unit time;
   2. variation of the sample mass per unit area;
   3. variation of the sample mass, per unit time;
   4. sample size variation per unit time;
5. In the gravimetric method, aluminum plate:
   1. is degreased in sodium hydroxide solution;
   2. is weighed before and after immersing it in NaOH;
   3. is weight only after immersion;
   4. is not necessary, weighing the aluminum sample;

Final laboratory test

Metal corrosion

1. The corrosion rate is:
   1. variation of the sample mass, per unit time;
   2. variation of the sample mass per unit area;
   3. sample size variation per unit time;
   4. variation of the sample mass per unit area, per unit time;
2. When calculating the corrosion rate the surface is expressed in:
   1. dm²;
   2. m³;;
   3. m²;
   4. cm²;
3. In corrosion processes studied gas is released:
   1. only the corrosion of zinc;
   2. which is a volume that depends on the amount of metal corroded;
   3. which is a volume that does not depend on the sample surface;
   4. only the corrosion of aluminum;
4. In the gravimetric method, aluminum plate:
   1. is weighed before and after immersing it in NaOH;
   2. is not necessary, weighing the aluminum sample;
   3. is degreased in sodium hydroxide solution;
   4. is weight only after immersion;
5. Resistance grouping of the two samples studied in the laboratory is based on:
   1. the surface of the samples;
   2. the value of penetration index;
   3. their mass;
   4. their size, and time that are subject to chemical agents;

Final laboratory test

Metal corrosion

1. Corrosion of metals is:
   1. the cleaning of metals;
   2. the protection in time to chemical agents;
   3. the destruction of metals under the action of external factors;
   4. a beneficial process that shows the stability of metals;
2. At the volumetric method:
   1. the sample size of zinc are measured, and then weighed the sample;
   2. weigh the zinc before and after the process takes place;
   3. is not required, weighing the sample of zinc;
   4. degrease the sample in sulfuric acid solution;
3. When calculating the corrosion rate the surface is expressed in:
   1. cm²;
   2. m³;;
   3. m²;
   4. dm²;
4. In corrosion processes studied gas is released:
   1. which is a volume that depends on the amount of metal corroded;
   2. which is a volume that does not depend on the sample surface;
   3. only the corrosion of aluminum;
   4. only the corrosion of zinc;
5. The corrosion rate is:
   1. variation of the sample mass per unit area;
   2. variation of the sample mass per unit area, per unit time;
   3. sample size variation per unit time;
   4. variation of the sample mass, per unit time;

Final laboratory test

Metal alloys analysis

1. When identify lead, is obtain a:
   1. blue complex;
   2. violet complex;
   3. red-brown complex;
   4. yellow complex;
2. The oxidation state, which pass into solution, analyzed metal ions are:
   1. Fe³⁺; Ni²⁺; Cu²⁺; Zn²⁺; Co²⁺; Cr³⁺
   2. Fe²⁺; Ni¹⁺; Cu¹⁺; Zn³⁺; Co²⁺; Cr⁶⁺
   3. dependent on the intensity of the current applied to the electrograf and composition of the metal alloy;
   4. Fe²⁺; Ni³⁺; Cu¹⁺; Zn³⁺; Co³⁺; Cr²⁺
3. The filter paper was acidified before analysis for:
   1. dissolution of hard soluble hydroxides;
   2. to remove the cations from the analyzed sample;
   3. dissolution of acids;
   4. to complex the cations from the sample;
4. When identify aluminum, ammonium hydroxide was added:
   1. for obtaining a red color complex;
   2. for ensuring the necessary pH, for the reaction;
   3. for stopping the reaction;
   4. for removing the ions of Al³⁺;
5. The electrograf consists of:
   1. current source and the sample;
   2. filter paper and the sample;
   3. current source and the filter paper;
   4. none of the answers are correct;

Final laboratory test

Metal alloys analysis

1. Why moisten the filter paper with solution of sodium nitrate?
   1. none of the answers are correct;
   2. for stopping the chemical reaction that takes place;
   3. to be cut easily with scissors;
   4. for the paper work as insulation;
2. The oxidation state, which pass into solution, analyzed metal ions are:
   1. Fe³⁺; Ni²⁺; Cu²⁺; Zn²⁺; Co²⁺; Cr³⁺
   2. Fe²⁺; Ni³⁺; Cu¹⁺; Zn³⁺; Co³⁺; Cr²⁺
   3. dependent on the intensity of the current applied to the electrograf and composition of the metal alloy;
   4. Fe²⁺; Ni¹⁺; Cu¹⁺; Zn³⁺; Co²⁺; Cr⁶⁺
3. When identify aluminum, ammonium hydroxide was added:
   1. for stopping the reaction;
   2. for obtaining a red color complex;
   3. for removing the ions of Al³⁺;
   4. for ensuring the necessary pH, for the reaction;
4. The filter paper was acidified before analysis for:
   1. to remove the cations from the analyzed sample;
   2. dissolution of acids;
   3. to complex the cations from the sample;
   4. dissolution of hard soluble hydroxides;
5. The electrograf consists of:
   1. current source and the sample;
   2. current source and the filter paper;
   3. none of the answers are correct;
   4. filter paper and the sample;

Final laboratory test

Metal alloys analysis

1. The electrograf consists of:
   1. none of the answers are correct;
   2. current source and the filter paper;
   3. current source and the sample;
   4. filter paper and the sample;
2. The oxidation state, which pass into solution, analyzed metal ions are:
   1. Fe³⁺; Ni²⁺; Cu²⁺; Zn²⁺; Co²⁺; Cr³⁺
   2. dependent on the intensity of the current applied to the electrograf and composition of the metal alloy;
   3. Fe²⁺; Ni¹⁺; Cu¹⁺; Zn³⁺; Co²⁺; Cr⁶⁺
   4. Fe²⁺; Ni³⁺; Cu¹⁺; Zn³⁺; Co³⁺; Cr²⁺
3. The filter paper was acidified before analysis for:
   1. to remove the cations from the analyzed sample;
   2. dissolution of hard soluble hydroxides;
   3. dissolution of acids;
   4. to complex the cations from the sample;
4. When identify lead, is obtain a:
   1. yellow complex;
   2. violet complex;
   3. blue complex;
   4. red-brown complex;
5. This method of analysis of metal alloys is:
   1. a nondestructive method of analysis;
   2. a quantitative method of analysis;
   3. destructive method of analysis;
   4. a gravimetric method of analysis;

Final laboratory test

Metal alloys analysis

1. When identify lead, is obtain a:
   1. blue complex;
   2. red-brown complex;
   3. violet complex;
   4. yellow complex;
2. The filter paper was acidified before analysis for:
   1. to remove the cations from the analyzed sample;
   2. dissolution of acids;
   3. to complex the cations from the sample;
   4. dissolution of hard soluble hydroxides;
3. This method of analysis of metal alloys is:
   1. destructive method of analysis;
   2. a nondestructive method of analysis;
   3. a gravimetric method of analysis;
   4. a quantitative method of analysis;
4. Why moisten the filter paper with solution of sodium nitrate?
   1. to be cut easily with scissors;
   2. for the paper work as insulation;
   3. none of the answers are correct;
   4. for stopping the chemical reaction that takes place;
5. The oxidation state, which pass into solution, analyzed metal ions are:
   1. dependent on the intensity of the current applied to the electrograf and composition of the metal alloy;
   2. Fe²⁺; Ni³⁺; Cu¹⁺; Zn³⁺; Co³⁺; Cr²⁺
   3. Fe²⁺; Ni¹⁺; Cu¹⁺; Zn³⁺; Co²⁺; Cr⁶⁺
   4. Fe³⁺; Ni²⁺; Cu²⁺; Zn²⁺; Co²⁺; Cr³⁺

Final laboratory test

Metal alloys analysis

1. This method of analysis of metal alloys is:
   1. a nondestructive method of analysis;
   2. a quantitative method of analysis;
   3. a gravimetric method of analysis;
   4. destructive method of analysis;
2. The filter paper was acidified before analysis for:
   1. dissolution of hard soluble hydroxides;
   2. dissolution of acids;
   3. to remove the cations from the analyzed sample;
   4. to complex the cations from the sample;
3. The oxidation state, which pass into solution, analyzed metal ions are:
   1. Fe²⁺; Ni³⁺; Cu¹⁺; Zn³⁺; Co³⁺; Cr²⁺
   2. Fe³⁺; Ni²⁺; Cu²⁺; Zn²⁺; Co²⁺; Cr³⁺
   3. Fe²⁺; Ni¹⁺; Cu¹⁺; Zn³⁺; Co²⁺; Cr⁶⁺
   4. dependent on the intensity of the current applied to the electrograf and composition of the metal alloy;
4. When identify lead, is obtain a:
   1. violet complex;
   2. red-brown complex;
   3. blue complex;
   4. yellow complex;
5. The electrograf consists of:
   1. current source and the sample;
   2. filter paper and the sample;
   3. none of the answers are correct;
   4. current source and the filter paper;

Final laboratory test

Protection of metals by nickelling

1. In the experiment of nickelling:
   1. with as nickel sulfate solution is more concentrated, the more nickel is deposited on the cathode;
   2. nickel sulfate solution is weakly electrically conductive;
   3. iron from the cathode move in solution, replacing the nickel to be deposited;
   4. nickel anode is consumed;
2. Plates, which shall be deposited nickel are incorporated into the electrolysis bath:
   1. as a cathode because at the cathode reduction processes take place;
   2. as a cathode because at the cathode oxidation processes take place;
   3. as the anode because at the anode oxidation processes take place;
   4. as the anode because at the anode reduction processes take place;
3. When is submitted the sample to the electrolysis process, this:
   1. is introduced in natrium chloride for degreasing;
   2. is introduced in milk of lime solution for degreasing;
   3. is inserted into sulfuric acid, to clean;
   4. degreasing is not necessary because the oil stains do not affect the electrolysis process;
4. Theoretical mass of nickel deposited is calculated using:
   1. none of the answers are correct;
   2. solutions laws;
   3. law of mass action;
   4. perfect gas law;
5. In order to determine porosity:
   1. degrease steel plate in potassium chloride;
   2. steel sample is cleaned with filter paper;
   3. include pores of the filter paper obtained by contact with steel plate;
   4. steel plate weigh;

Final laboratory test

Protection of metals by nickelling

1. An electrolysis cell consists of:
   1. the anode, cathode, electrolyte solution, current source;
   2. two electrodes and filter paper;
   3. the anode, cathode, and samples;
   4. analysis samples and electrolyte solution;
2. Plates, which shall be deposited nickel are incorporated into the electrolysis bath:
   1. as the anode because at the anode oxidation processes take place;
   2. as the anode because at the anode reduction processes take place;
   3. as a cathode because at the cathode reduction processes take place;
   4. as a cathode because at the cathode oxidation processes take place;
3. Theoretical mass of nickel deposited is calculated using:
   1. law of mass action;
   2. solutions laws;
   3. none of the answers are correct;
   4. perfect gas law;
4. In order to determine porosity:
   1. include pores of the filter paper obtained by contact with steel plate;
   2. steel sample is cleaned with filter paper;
   3. degrease steel plate in potassium chloride;
   4. steel plate weigh;
5. When is submitted the sample to the electrolysis process, this:
   1. is introduced in milk of lime solution for degreasing;
   2. degreasing is not necessary because the oil stains do not affect the electrolysis process;
   3. is inserted into sulfuric acid, to clean;
   4. is introduced in natrium chloride for degreasing;

Final laboratory test

Protection of metals by nickelling

1. Plates, which shall be deposited nickel are incorporated into the electrolysis bath:
   1. as the anode because at the anode reduction processes take place;
   2. as a cathode because at the cathode oxidation processes take place;
   3. as the anode because at the anode oxidation processes take place;
   4. as a cathode because at the cathode reduction processes take place;
2. In the experiment of nickelling:
   1. with as nickel sulfate solution is more concentrated, the more nickel is deposited on the cathode;
   2. nickel anode is consumed;
   3. nickel sulfate solution is weakly electrically conductive;
   4. iron from the cathode move in solution, replacing the nickel to be deposited;
3. Theoretical mass of nickel deposited is calculated using:
   1. law of mass action;
   2. none of the answers are correct;
   3. solutions laws;
   4. perfect gas law;
4. To determine the current efficiency, brass plate:
   1. is degreased in sulfuric acid;
   2. it is not required, weighing the plate because is determined the porosity of this sample;
   3. is weighed only after the electrolysis process takes place;
   4. is weighed before and after immersion in the electrolytic bath;
5. When is submitted the sample to the electrolysis process, this:
   1. is introduced in natrium chloride for degreasing;
   2. is introduced in milk of lime solution for degreasing;
   3. degreasing is not necessary because the oil stains do not affect the electrolysis process;
   4. is inserted into sulfuric acid, to clean;

Final laboratory test

Protection of metals by nickelling

1. An electrolysis cell consists of:
   1. the anode, cathode, electrolyte solution, current source;
   2. the anode, cathode, and samples;
   3. analysis samples and electrolyte solution;
   4. two electrodes and filter paper;
2. To determine the current efficiency, brass plate:
   1. it is not required, weighing the plate because is determined the porosity of this sample;
   2. is degreased in sulfuric acid;
   3. is weighed only after the electrolysis process takes place;
   4. is weighed before and after immersion in the electrolytic bath;
3. Plates, which shall be deposited nickel are incorporated into the electrolysis bath:
   1. as a cathode because at the cathode reduction processes take place;
   2. as the anode because at the anode oxidation processes take place;
   3. as a cathode because at the cathode oxidation processes take place;
   4. as the anode because at the anode reduction processes take place;
4. Theoretical mass of nickel deposited is calculated using:
   1. law of mass action;
   2. solutions laws;
   3. perfect gas law;
   4. none of the answers are correct;
5. When is submitted the sample to the electrolysis process, this:
   1. degreasing is not necessary because the oil stains do not affect the electrolysis process;
   2. is inserted into sulfuric acid, to clean;
   3. is introduced in milk of lime solution for degreasing;
   4. is introduced in natrium chloride for degreasing;

Final laboratory test

Protection of metals by nickelling

1. When is submitted the sample to the electrolysis process, this:
   1. is inserted into sulfuric acid, to clean;
   2. is introduced in natrium chloride for degreasing;
   3. degreasing is not necessary because the oil stains do not affect the electrolysis process;
   4. is introduced in milk of lime solution for degreasing;
2. Plates, which shall be deposited nickel are incorporated into the electrolysis bath:
   1. as a cathode because at the cathode reduction processes take place;
   2. as a cathode because at the cathode oxidation processes take place;
   3. as the anode because at the anode reduction processes take place;
   4. as the anode because at the anode oxidation processes take place;
3. In order to determine porosity:
   1. steel plate weigh;
   2. degrease steel plate in potassium chloride;
   3. steel sample is cleaned with filter paper;
   4. include pores of the filter paper obtained by contact with steel plate;
4. Theoretical mass of nickel deposited is calculated using:
   1. perfect gas law;
   2. law of mass action;
   3. none of the answers are correct;
   4. solutions laws;
5. In the experiment of nickelling:
   1. with as nickel sulfate solution is more concentrated, the more nickel is deposited on the cathode;
   2. nickel sulfate solution is weakly electrically conductive;
   3. nickel anode is consumed;
   4. iron from the cathode move in solution, replacing the nickel to be deposited;

Final laboratory test

The study of difusion in gazeous state and molecular rates

1. Which of the models studied approximates best diffusion:
   1. speeds and/or energy mean;
   2. speeds and/or energy to fashion;
   3. speeds and/or quadratic energy;
   4. none of the answers are correct;
2. The diffusion model of the two species (NH₃ and HCl) is chosen as follows:
   1. identify the largest absolute difference between gear ratios;
   2. identify the smallest absolute difference between gear ratios;
   3. identify the largest absolute difference between diffusion coefficients ratios;
   4. not distinguish between gear ratios because it shows no importance;
3. Measuring the distances, is as follows:
   1. none of the answers are correct;
   2. from the two spots with HCl and NH₃ respectively, to form NH₄Cl ring;
   3. from the two ends of the glass tube, to the form ring;
   4. from the two rubber plugs to the ring formed;
4. For accurate measurement of diffusion time:
   1. the two pads moistened are introduced at a certain time, into the glass tube and then stop the timer;
   2. the two pads moistened are introduced simultaneously in the glass tube and start the timer;
   3. the two pads moistened, placed on line, in the glass tube and start the timer;
   4. the two pads moistened are introduced simultaneously in the glass tube and stop the timer;
5. After NH₃ and HCl molecules diffuse:
   1. must be clean the tube to leave the workplace clean;
   2. the gas discharge occurs in the tube;
   3. all other answers are correct;
   4. there is a chemical reaction to form ammonium chloride (NH₄Cl);

Final laboratory test

The study of difusion in gazeous state and molecular rates

1. Which parameters were identical, at the diffusion, of NH₃ and HCl:
   1. temperature and concentration;
   2. the weigh of pads and concentration;
   3. temperature and time of diffusion;
   4. the time of diffusion and concentration;
2. For accurate measurement of diffusion time:
   1. the two pads moistened, placed on line, in the glass tube and start the timer;
   2. the two pads moistened are introduced at a certain time, into the glass tube and then stop the timer;
   3. the two pads moistened are introduced simultaneously in the glass tube and start the timer;
   4. the two pads moistened are introduced simultaneously in the glass tube and stop the timer;
3. Measuring the distances, is as follows:
   1. from the two ends of the glass tube, to the form ring;
   2. none of the answers are correct;
   3. from the two spots with HCl and NH₃ respectively, to form NH₄Cl ring;
   4. from the two rubber plugs to the ring formed;
4. The diffusion model of the two species (NH₃ and HCl) is chosen as follows:
   1. not distinguish between gear ratios because it shows no importance;
   2. identify the smallest absolute difference between gear ratios;
   3. identify the largest absolute difference between gear ratios;
   4. identify the largest absolute difference between diffusion coefficients ratios;
5. Diffusion rates are calculated from:
   1. measured distances and time report;
   2. diffusion coefficients and time report;
   3. molecular speeds and energies media report;
   4. average energy and time report;

Final laboratory test

The study of difusion in gazeous state and molecular rates

1. Which of the models studied approximates best diffusion:
   1. speeds and/or energy mean;
   2. speeds and/or quadratic energy;
   3. none of the answers are correct;
   4. speeds and/or energy to fashion;
2. Which parameters were identical, at the diffusion, of NH₃ and HCl:
   1. the weigh of pads and concentration;
   2. temperature and time of diffusion;
   3. the time of diffusion and concentration;
   4. temperature and concentration;
3. For accurate measurement of diffusion time:
   1. the two pads moistened, placed on line, in the glass tube and start the timer;
   2. the two pads moistened are introduced simultaneously in the glass tube and stop the timer;
   3. the two pads moistened are introduced at a certain time, into the glass tube and then stop the timer;
   4. the two pads moistened are introduced simultaneously in the glass tube and start the timer;
4. The diffusion model of the two species (NH₃ and HCl) is chosen as follows:
   1. not distinguish between gear ratios because it shows no importance;
   2. identify the largest absolute difference between diffusion coefficients ratios;
   3. identify the smallest absolute difference between gear ratios;
   4. identify the largest absolute difference between gear ratios;
5. After NH₃ and HCl molecules diffuse:
   1. the gas discharge occurs in the tube;
   2. there is a chemical reaction to form ammonium chloride (NH₄Cl);
   3. all other answers are correct;
   4. must be clean the tube to leave the workplace clean;

Final laboratory test

The study of difusion in gazeous state and molecular rates

1. Measuring the distances, is as follows:
   1. from the two ends of the glass tube, to the form ring;
   2. from the two spots with HCl and NH₃ respectively, to form NH₄Cl ring;
   3. from the two rubber plugs to the ring formed;
   4. none of the answers are correct;
2. Which parameters were identical, at the diffusion, of NH₃ and HCl:
   1. the time of diffusion and concentration;
   2. the weigh of pads and concentration;
   3. temperature and time of diffusion;
   4. temperature and concentration;
3. The diffusion model of the two species (NH₃ and HCl) is chosen as follows:
   1. identify the smallest absolute difference between gear ratios;
   2. not distinguish between gear ratios because it shows no importance;
   3. identify the largest absolute difference between gear ratios;
   4. identify the largest absolute difference between diffusion coefficients ratios;
4. Which of the models studied approximates best diffusion:
   1. none of the answers are correct;
   2. speeds and/or quadratic energy;
   3. speeds and/or energy to fashion;
   4. speeds and/or energy mean;
5. After NH₃ and HCl molecules diffuse:
   1. the gas discharge occurs in the tube;
   2. must be clean the tube to leave the workplace clean;
   3. all other answers are correct;
   4. there is a chemical reaction to form ammonium chloride (NH₄Cl);

Final laboratory test

The study of difusion in gazeous state and molecular rates

1. Diffusion rates are calculated from:
   1. measured distances and time report;
   2. molecular speeds and energies media report;
   3. diffusion coefficients and time report;
   4. average energy and time report;
2. Which of the models studied approximates best diffusion:
   1. speeds and/or energy to fashion;
   2. none of the answers are correct;
   3. speeds and/or energy mean;
   4. speeds and/or quadratic energy;
3. Measuring the distances, is as follows:
   1. from the two spots with HCl and NH₃ respectively, to form NH₄Cl ring;
   2. from the two rubber plugs to the ring formed;
   3. from the two ends of the glass tube, to the form ring;
   4. none of the answers are correct;
4. For accurate measurement of diffusion time:
   1. the two pads moistened are introduced simultaneously in the glass tube and stop the timer;
   2. the two pads moistened are introduced simultaneously in the glass tube and start the timer;
   3. the two pads moistened, placed on line, in the glass tube and start the timer;
   4. the two pads moistened are introduced at a certain time, into the glass tube and then stop the timer;
5. After NH₃ and HCl molecules diffuse:
   1. there is a chemical reaction to form ammonium chloride (NH₄Cl);
   2. the gas discharge occurs in the tube;
   3. all other answers are correct;
   4. must be clean the tube to leave the workplace clean;