Question 1

The capacity of a battery usually is specified in units of amperes $\bullet$ hours.Show that with this information and the voltage of the battery, you can determine the amount of energy that can be obtained from the battery.

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Question 2

A single cell in a lead acid battery produces 2.0 V and is constructed based on a chemical process that involves the transfer of 2 electrons from anode to cathode per reaction.What is the change in free energy?

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Question 3

What is the most important use for a standard hydrogen electrode?

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Question 4

Suppose a NiMH battery is rated as 1.20 V and 1.50 A•hr.Assuming one mole of electrons is transferred per mole of reaction, approximately how many grams of NiOOH) 91.70 g/mol) are required to make this battery? How much electrical energy can this battery provide? MH +NiOOH) $\rightarrow$ M +(NiOH)₂

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Question 5

How many coulombs of charge are transferred per mole of reaction in an electrochemical cell using the following reaction? 2 Cr³⁺(aq) + 3 Zn(s) $\rightarrow$2 Cr(s)+ 3 Zn²⁺(aq)

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Question 6

A concentration cell is made using Ni²⁺solutions and Ni electrodes.In one compartment, [Ni²⁺] = 1.00 M; in the other, [Ni²⁺] is due to the dissolution of Ni(OH)₂ in an aqueous solution buffered to a pH of 13.000.The measured E_cell at 298 K is 0.4038 V.Find the concentration of Ni²⁺in the saturated Ni(OH)₂ solution, and calculate an estimate of K_sp for nickel hydroxide.

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Question 7

How does a fuel cell differ from a conventional battery?

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Question 8

Based on the information in the table of standard reduction potentials below, explain what, if anything, will happen if iodine is placed in an aqueous solution containing bromide ions.

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Question 9

What is the electrical work that can be done in an electrochemical cell using the following half-reactions under standard state?

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Question 10

The capacity of a battery usually is specified in units of amperes $\bullet$ hours.Show that these units are actually propertional to the number of electrons that can be supplied by the battery.

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Question 11

If, in using a lead-acid battery to start a car, 1.00 g of Pb is consumed on the anode, how long will it take to recharge the battery using a current of 0.500 amps and to turn the PbSO₄ that was produced back into Pb?

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Question 12

A 1.5 V alkaline battery is constructed based on a chemical process that involves the transfer of 2 electrons from anode to cathode per reaction.How much work can be done?

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Question 13

Starting with $\Delta$G =$\Delta$G° + RT ln Q and $\Delta$G = -nFE, derive the Nernst equation.

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Question 14

What constitutes a standard hydrogen electrode?

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Question 15

Chromium often is electroplated on other metals and even plastics to produce a shiny metallic appearance.How many grams of chromium would plate out from a solution of Cr(NO₃)₃ when 15.0 amps of current are passed through the electrolytic cell for 4.50 hours?

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Quiz 17: Electrochemistry the Quest for Clean Energy

The capacity of a battery usually is specified in units of amperes $\bullet$ hours.Show that with this information and the voltage of the battery, you can determine the amount of energy that can be obtained from the battery.

A single cell in a lead acid battery produces 2.0 V and is constructed based on a chemical process that involves the transfer of 2 electrons from anode to cathode per reaction.What is the change in free energy?

What is the most important use for a standard hydrogen electrode?

How many coulombs of charge are transferred per mole of reaction in an electrochemical cell using the following reaction? 2 Cr³⁺(aq) + 3 Zn(s) $\rightarrow$ 2 Cr(s)+ 3 Zn²⁺(aq)

How does a fuel cell differ from a conventional battery?

Based on the information in the table of standard reduction potentials below, explain what, if anything, will happen if iodine is placed in an aqueous solution containing bromide ions.

What is the electrical work that can be done in an electrochemical cell using the following half-reactions under standard state?

The capacity of a battery usually is specified in units of amperes $\bullet$ hours.Show that these units are actually propertional to the number of electrons that can be supplied by the battery.

If, in using a lead-acid battery to start a car, 1.00 g of Pb is consumed on the anode, how long will it take to recharge the battery using a current of 0.500 amps and to turn the PbSO₄ that was produced back into Pb?

A 1.5 V alkaline battery is constructed based on a chemical process that involves the transfer of 2 electrons from anode to cathode per reaction.How much work can be done?

Starting with $\Delta$ G = $\Delta$ G° + RT ln Q and $\Delta$ G = -nFE, derive the Nernst equation.

What constitutes a standard hydrogen electrode?

Chromium often is electroplated on other metals and even plastics to produce a shiny metallic appearance.How many grams of chromium would plate out from a solution of Cr(NO₃)₃ when 15.0 amps of current are passed through the electrolytic cell for 4.50 hours?

Quiz 17: Electrochemistry the Quest for Clean Energy

The capacity of a battery usually is specified in units of amperes ∙\bullet∙ hours.Show that with this information and the voltage of the battery, you can determine the amount of energy that can be obtained from the battery.

A single cell in a lead acid battery produces 2.0 V and is constructed based on a chemical process that involves the transfer of 2 electrons from anode to cathode per reaction.What is the change in free energy?

What is the most important use for a standard hydrogen electrode?

How many coulombs of charge are transferred per mole of reaction in an electrochemical cell using the following reaction? 2 Cr3+(aq) + 3 Zn(s) →\rightarrow→ 2 Cr(s)+ 3 Zn2+(aq)

How does a fuel cell differ from a conventional battery?

Based on the information in the table of standard reduction potentials below, explain what, if anything, will happen if iodine is placed in an aqueous solution containing bromide ions.

What is the electrical work that can be done in an electrochemical cell using the following half-reactions under standard state?

The capacity of a battery usually is specified in units of amperes ∙\bullet∙ hours.Show that these units are actually propertional to the number of electrons that can be supplied by the battery.

If, in using a lead-acid battery to start a car, 1.00 g of Pb is consumed on the anode, how long will it take to recharge the battery using a current of 0.500 amps and to turn the PbSO4 that was produced back into Pb?

A 1.5 V alkaline battery is constructed based on a chemical process that involves the transfer of 2 electrons from anode to cathode per reaction.How much work can be done?

Starting with Δ\DeltaΔ G = Δ\DeltaΔ G° + RT ln Q and Δ\DeltaΔ G = -nFE, derive the Nernst equation.

What constitutes a standard hydrogen electrode?

Chromium often is electroplated on other metals and even plastics to produce a shiny metallic appearance.How many grams of chromium would plate out from a solution of Cr(NO3)3 when 15.0 amps of current are passed through the electrolytic cell for 4.50 hours?

The capacity of a battery usually is specified in units of amperes $\bullet$ hours.Show that with this information and the voltage of the battery, you can determine the amount of energy that can be obtained from the battery.

How many coulombs of charge are transferred per mole of reaction in an electrochemical cell using the following reaction? 2 Cr³⁺(aq) + 3 Zn(s) $\rightarrow$ 2 Cr(s)+ 3 Zn²⁺(aq)

The capacity of a battery usually is specified in units of amperes $\bullet$ hours.Show that these units are actually propertional to the number of electrons that can be supplied by the battery.

If, in using a lead-acid battery to start a car, 1.00 g of Pb is consumed on the anode, how long will it take to recharge the battery using a current of 0.500 amps and to turn the PbSO₄ that was produced back into Pb?

Starting with $\Delta$ G = $\Delta$ G° + RT ln Q and $\Delta$ G = -nFE, derive the Nernst equation.

Chromium often is electroplated on other metals and even plastics to produce a shiny metallic appearance.How many grams of chromium would plate out from a solution of Cr(NO₃)₃ when 15.0 amps of current are passed through the electrolytic cell for 4.50 hours?