Question 1

An electroplating solution is made up of nickel(II)sulfate. How much time would it take to deposit 0.500 g of metallic nickel on a custom car part using a current of 3.00 A?

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Question 2

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M)$\rarr$Fe²⁺(1.0 M)+ Sn. Sketch a diagram of such a cell. Be sure to label the anode and cathode, and show the direction of electron flow in the external circuit. Write the half-reactions occurring at the electrodes.

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Question 3

You wish to electroplate a metal utensil with a surface area of 736 cm² with gold to give an average thickness of 0.025 mm over the entire surface. Starting with a solution of excess Au³⁺ and applying a constant current of 14 A, how long will it take to electroplate the utensil? The density of gold is 19.3 g/cm³.

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Question 4

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl₂(g)is evolved at the anode.

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During the electrolysis of an aqueous solution of NaCl, hydrogen gas (H2) is produced at the cathode (due to the reduction of water), and chlorine gas (Cl2) is evolved at the anode, not sodium metal (Na).

Question 5

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl₂. If E_cell is found to be 0.24 V, what is the pH of the acetic acid solution?

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Question 6

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

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Question 7

Consider the reaction Fe + Sn²⁺(1 *10^-3 M)$\rarr$Fe²⁺(1.0 M)+ Sn. Calculate the voltage theoretically generated by the cell.

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Question 8

Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm)$\rarr$ 2Ag(s)+ 2H⁺(pH = 6.0)

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Question 9

Many different ways have been proposed to make batteries. One cell is set up with copper and lead electrodes in contact with CuSO₄(aq)and Pb(NO₃)₂ (aq), respectively. If the Pb²⁺ and Cu²⁺concentrations are each 1.0 M, what is the overall cell potential? Pb²⁺ + 2e^- $\rarr$Pb E° = -0.22 V Cu²⁺ + 2e^- $\rarr$ Cu E° = +0.34 V

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Question 10

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq)using a current of 6.0 A?

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Question 11

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M)$\rarr$Fe²⁺(1.0 M)+ Sn. In what direction do the Cl^- ions in the KCl salt bridge flow?

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Question 12

What concentration of Ni²⁺ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO₄ solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

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Question 13

In an electrolytic cell, electrical energy is used to cause a chemical reaction to occur that would otherwise be nonspontaneous.

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In an electrolytic cell, an external voltage is applied to cause a nonspontaneous reaction to occur. This requires an input of electrical energy.

Question 14

The reduction of 1.00 mole of Cr³⁺ to Cr requires 9.65 *10⁴ C of electrical charge.

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Question 15

The electrochemical cell that utilizes the reaction Zn + Cu²⁺(1 M)$\rarr$Zn²⁺(1 M)+ Cu will have a lower cell emf when the concentrations of Zn²⁺ and Cu²⁺ ions are decreased to 0.1 M.

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Question 16

How many moles of H₂ are producedby 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 10² s?

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Question 17

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO₄(aq)and Pb(NO₃)₂ (aq)solutions, respectively. If sulfuric acid is then added to the Pb(NO₃)₂ solution, thereby forming a precipitate of PbSO₄, what will happen to the cell potential?

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Question 18

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO₄ for a period of 19.0 min?

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Quiz 19: Redox Reactions and Electrochemistry

An electroplating solution is made up of nickel(II)sulfate. How much time would it take to deposit 0.500 g of metallic nickel on a custom car part using a current of 3.00 A?

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M) $\rarr$ Fe²⁺(1.0 M)+ Sn. Sketch a diagram of such a cell. Be sure to label the anode and cathode, and show the direction of electron flow in the external circuit. Write the half-reactions occurring at the electrodes.

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl₂(g)is evolved at the anode.

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl₂. If E_cell is found to be 0.24 V, what is the pH of the acetic acid solution?

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Consider the reaction Fe + Sn²⁺(1 *10^-3 M) $\rarr$ Fe²⁺(1.0 M)+ Sn. Calculate the voltage theoretically generated by the cell.

Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm) $\rarr$ 2Ag(s)+ 2H⁺(pH = 6.0)

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq)using a current of 6.0 A?

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M) $\rarr$ Fe²⁺(1.0 M)+ Sn. In what direction do the Cl^- ions in the KCl salt bridge flow?

What concentration of Ni²⁺ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO₄ solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

In an electrolytic cell, electrical energy is used to cause a chemical reaction to occur that would otherwise be nonspontaneous.

The reduction of 1.00 mole of Cr³⁺ to Cr requires 9.65 *10⁴ C of electrical charge.

The electrochemical cell that utilizes the reaction Zn + Cu²⁺(1 M) $\rarr$ Zn²⁺(1 M)+ Cu will have a lower cell emf when the concentrations of Zn²⁺ and Cu²⁺ ions are decreased to 0.1 M.

How many moles of H₂ are producedby 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 10² s?

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO₄(aq)and Pb(NO₃)₂ (aq)solutions, respectively. If sulfuric acid is then added to the Pb(NO₃)₂ solution, thereby forming a precipitate of PbSO₄, what will happen to the cell potential?

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO₄ for a period of 19.0 min?

Quiz 19: Redox Reactions and Electrochemistry

An electroplating solution is made up of nickel(II)sulfate. How much time would it take to deposit 0.500 g of metallic nickel on a custom car part using a current of 3.00 A?

Consider the reaction Fe + Sn2+(1 * 10-3 M) →\rarr→ Fe2+(1.0 M)+ Sn. Sketch a diagram of such a cell. Be sure to label the anode and cathode, and show the direction of electron flow in the external circuit. Write the half-reactions occurring at the electrodes.

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl2(g)is evolved at the anode.

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl2. If Ecell is found to be 0.24 V, what is the pH of the acetic acid solution?

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Consider the reaction Fe + Sn2+(1 *10-3 M) →\rarr→ Fe2+(1.0 M)+ Sn. Calculate the voltage theoretically generated by the cell.

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M)+ H2(1 atm) →\rarr→ 2Ag(s)+ 2H+(pH = 6.0)

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq)using a current of 6.0 A?

Consider the reaction Fe + Sn2+(1 * 10-3 M) →\rarr→ Fe2+(1.0 M)+ Sn. In what direction do the Cl- ions in the KCl salt bridge flow?

What concentration of Ni2+ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO4 solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

In an electrolytic cell, electrical energy is used to cause a chemical reaction to occur that would otherwise be nonspontaneous.

The reduction of 1.00 mole of Cr3+ to Cr requires 9.65 *104 C of electrical charge.

The electrochemical cell that utilizes the reaction Zn + Cu2+ (1 M) →\rarr→ Zn2+ (1 M)+ Cu will have a lower cell emf when the concentrations of Zn2+ and Cu2+ ions are decreased to 0.1 M.

How many moles of H2 are produced by 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 102 s?

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO4(aq)and Pb(NO3)2 (aq)solutions, respectively. If sulfuric acid is then added to the Pb(NO3)2 solution, thereby forming a precipitate of PbSO4, what will happen to the cell potential?

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO4 for a period of 19.0 min?

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M) $\rarr$ Fe²⁺(1.0 M)+ Sn. Sketch a diagram of such a cell. Be sure to label the anode and cathode, and show the direction of electron flow in the external circuit. Write the half-reactions occurring at the electrodes.

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl₂(g)is evolved at the anode.

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl₂. If E_cell is found to be 0.24 V, what is the pH of the acetic acid solution?

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Consider the reaction Fe + Sn²⁺(1 *10^-3 M) $\rarr$ Fe²⁺(1.0 M)+ Sn. Calculate the voltage theoretically generated by the cell.

Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm) $\rarr$ 2Ag(s)+ 2H⁺(pH = 6.0)

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq)using a current of 6.0 A?

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M) $\rarr$ Fe²⁺(1.0 M)+ Sn. In what direction do the Cl^- ions in the KCl salt bridge flow?

What concentration of Ni²⁺ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO₄ solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

The reduction of 1.00 mole of Cr³⁺ to Cr requires 9.65 *10⁴ C of electrical charge.

The electrochemical cell that utilizes the reaction Zn + Cu²⁺(1 M) $\rarr$ Zn²⁺(1 M)+ Cu will have a lower cell emf when the concentrations of Zn²⁺ and Cu²⁺ ions are decreased to 0.1 M.

How many moles of H₂ are producedby 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 10² s?

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO₄(aq)and Pb(NO₃)₂ (aq)solutions, respectively. If sulfuric acid is then added to the Pb(NO₃)₂ solution, thereby forming a precipitate of PbSO₄, what will happen to the cell potential?

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO₄ for a period of 19.0 min?