Question 19.5: Calculating a Standard Free-Energy Change from a Standard Ce...

Calculating a Standard Free-Energy Change from a Standard Cell Potential
The standard cell potential at 25 °C is 0.90 V for the reaction

$2 Al(s) + 3 Zn^{2+}(aq) → 2 Al^{3+}(aq) + 3 Zn(s)$

Calculate the standard free-energy change for this reaction at 25 °C.

STRATEGY
To calculate $∆G°$ , we use the equation ∆G° = -nFE°, where n can be determined from the balanced chemical equation, F is $96,500 C/mol e^{-}$ , and E° is given.

IDENTIFY

Known	Unknown
Standard cell potential (E° = 0.90 V)	Standard free-energy change(∆G°)

The "Step-by-Step Explanation" refers to a detailed and sequential breakdown of the solution or reasoning behind the answer. This comprehensive explanation walks through each step of the answer, offering you clarity and understanding.
Our explanations are based on the best information we have, but they may not always be right or fit every situation.

The blue check mark means that this solution has been answered and checked by an expert. This guarantees that the final answer is accurate.
Learn more on how we answer questions.

This Question has been Answered.

Already have an account?

Related Answered Questions

Question: 19.13

calculating the amount of product produced by Electrolysis A constant current of 30.0 A is passed through an aqueous solution of NaCl for 1.00 h. How many grams of NaOH and how many liters of Cl2 gas at STP are produced? ...

Verified Answer:

Because electrons can be thought of as a reactant ...

Question: 19.12

Using Standard Reduction Potentials to Calculate an Equilibrium Constant Use the standard reduction potentials in Table 19.1 to calculate the equilibrium constant at 25 °C for the reaction 6 Br^-(aq) + Cr2O7^2-(aq) + 14 H^+(aq) → 3 Br2(aq) + 2 Cr^3+(aq) + 7 H2O(l) ...

Verified Answer:

Find the relevant half-reactions in Table 19.1, an...

Question: 19.11

Using the Nernst Equation in the Electrochemical Determination of ph The following cell has a potential of 0.55 V at 25 °C: Pt(s) | H2(1 atm) H^+(? M) || Cl^-(1 M) | Hg2Cl2(s) | Hg(l) What is the pH of the solution in the anode compartment? ...

Verified Answer:

The cell reaction is

H_{2}(g) + Hg_{2}Cl_{...

Question: 19.6

Arranging Oxidizing and Reducing Agents in Order of Increasing Strength (a) Arrange the following oxidizing agents in order of increasing strength under standard-state conditions: Br2(aq), Fe^3+(aq), Cr2O7^2-(aq). (b) Arrange the following reducing agents in order of increasing strength under ...

Verified Answer:

(a) List the half-reactions that involve

Br...

Question: 19.7

Predicting Whether a Redox Reaction Is Spontaneous Predict from Table 19.1 whether Pb^2+(aq) can oxidize Al(s) or Cu(s) under standardstate conditions. Calculate E° for each reaction at 25 °C. ...

Verified Answer:

Pb^{2+}(aq)

is above Al(s) in the t...

Question: 19.8

Calculating the Voltage of a Galvanic Cell under Standard-State Conditions What is the voltage of the galvanic cell shown in the illustration? What is the anode halfreaction, and what is the cathode half-reaction? Which direction do the electrons flow? ...

Verified Answer:

Table 19.1 gives the standard reduction potentials...

Question: 19.9

Using the Nernst Equation to Calculate the Cell Potential under Nonstandard-State Conditions Consider a galvanic cell that uses the reaction Zn(s) + 2 H^+(aq) → Zn^2+(aq) + H2(g) Calculate the cell potential at 25 °C when [H^+] = 1.0 M, [Zn^2+] = 0.0010 M, and PH2 = 0.10 atm. ...

Verified Answer:

The standard cell potential is

E° = E°_{Zn→...

Question: 19.10

Exploring How Changes in Concentrations Affect Cell Voltage Consider the following galvanic cell: (a) What is the change in the cell voltage on increasing the ion concentrations in the anode compartment by a factor of 10?(b) What is the change in the cell voltage on increasing the ion ...

Verified Answer:

(a)

Pb^{2+}

is in the anode compart...

Question: 19.4

Interpreting the Shorthand Notation for a Galvanic Cell Given the following shorthand notation Pt(s) | Sn^2+(aq), Sn^4+(aq) || Ag^+(aq) | Ag(s) write a balanced equation for the cell reaction, and give a brief description of the cell ...

Verified Answer:

Because the anode always appears at the left in th...

Question: 19.2

Balancing a Redox Equation for a Reaction in Basic Solution Aqueous sodium hypochlorite (NaOCl; household bleach) is a strong oxidizing agent that reacts with [Cr(OH)4^-]in basic solution to yield (CrO4^2-) and chloride ion. The net ionic equation is ClO^- (aq) + Cr(OH)4^-(aq) → CrO4^2-(aq)+Cl^-1 ...

Verified Answer:

Step 1. Write the unbalanced net ionic equation. [...