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A. -0.85V D. -2.37V B. +0.85V 8. Use the Table of Standard Reduction Potential Stable,which Species Would Reac with Al^3+ A. Pb Only C.

Question

a. -0.85V d. -2.37V b. +0.85V 8. Use the Table of Standard Reduction Potential stable,which species would reac with Al^3+ a. Pb only C. Fe and Pb b. Au^3- only d. Both Mg and k 9. The oxidation of hydrogen by oxygen is one of the most-used reactions in fuel. cell technology. The overall reaction which is given below,has a Delta G^circ value of -474kJ/mol What is the standard cell potential for this fuel cell? 2H_(2)(g)+O_(2)(g)arrow 2H_(2)O(l)Delta G^circ =-474kJ/mol a. 2.46V C. 1.23V b. 4.91 V d. 2.46 V 10. Which one of the following equations shows the relationship between standard Gibbs free energy and equilibrium constant? a. K=Delta G^circ C. Delta G^0=-RTlnK b. K=RTlnDelta G^circ d. Delta G^0=RTlnK 11. What is Delta G^circ for the following balanced reaction, if E^ast =+2.431V Al(s)+Fe^2ast (aq)arrow Al^3++Fe(l)E^ast =+2.431V a. -704kJ/mol b. +704kJ/mol C. -235kJ/mol d. -469kJ/mol 12. The value of E^ast for the following reaction is 1.10 V.What is the value of E_(ow) when the concentration of Cu^2+ is 1.0 M and the concentration of Zn^2+ is 0.025 M? Zn(s)+Cu^2+(aq)arrow Cu(s)+Zn^2+(aq)E^2=1.10 V.[Cu^2+]=1.0M [Zn^2+]=0.025M and a. 1.40 V b. 0.95 V C. 1.15V d. 0.80 V

Answer

4 (215 Votes)
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Dylan Advanced · Tutor for 1 years

Answer

For question 8, the answer depends on the specific reduction potentials of the species in the Table of Standard Reduction Potentials, which is not provided.For question 9, the answer is , so the answer is (a) 2.46 V.For question 10, the answer is (c) .For question 11, the answer is , so the answer is (a) -704 kJ/mol.For question 12, the answer depends on the specific temperature and reaction quotient, which are not provided.

Explanation

## Step 1: For question 8, we need to understand that a species will react with Al if it has a lower reduction potential than Al. By referring to the Table of Standard Reduction Potentials, we can determine which species have lower reduction potentials than Al.## Step 2: For question 9, we can use the formula for Gibbs free energy to calculate the standard cell potential. The formula is:### where is the Gibbs free energy, is the number of moles of electrons transferred, is the Faraday constant (96485 C/mol), and is the standard cell potential. We can rearrange this formula to solve for :### ## Step 3: For question 10, the correct relationship between standard Gibbs free energy and equilibrium constant is given by the formula:### where is the gas constant, is the temperature in Kelvin, and is the equilibrium constant.## Step 4: For question 11, we can use the formula for Gibbs free energy to calculate . The formula is:### where is the Gibbs free energy, is the number of moles of electrons transferred, is the Faraday constant (96485 C/mol), and is the standard cell potential.## Step 5: For question 12, we can use the Nernst equation to calculate . The Nernst equation is:### where is the cell potential, is the standard cell potential, is the gas constant, is the temperature in Kelvin, is the number of moles of electrons transferred, is the Faraday constant (96485 C/mol), and is the reaction quotient.