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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. 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

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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. 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

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

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DylanAdvanced · Tutor for 1 years

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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.<br /><br />For question 9, the answer is \(E^{\circ} = -\frac{-474 \times 10^3}{2 \times 96485} = 2.46 V\), so the answer is (a) 2.46 V.<br /><br />For question 10, the answer is (c) \(\Delta G^{0} = -RT\ln K\).<br /><br />For question 11, the answer is \(\Delta G^{\circ} = -3 \times 96485 \times 2.431 = -704 kJ/mol\), so the answer is (a) -704 kJ/mol.<br /><br />For question 12, the answer depends on the specific temperature and reaction quotient, which are not provided.

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## Step 1: <br />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.<br /><br />## Step 2: <br />For question 9, we can use the formula for Gibbs free energy to calculate the standard cell potential. The formula is:<br /><br />### \(\Delta G^{\circ} = -nFE^{\circ}\)<br /><br />where \(\Delta G^{\circ}\) is the Gibbs free energy, \(n\) is the number of moles of electrons transferred, \(F\) is the Faraday constant (96485 C/mol), and \(E^{\circ}\) is the standard cell potential. We can rearrange this formula to solve for \(E^{\circ}\):<br /><br />### \(E^{\circ} = -\frac{\Delta G^{\circ}}{nF}\)<br /><br />## Step 3: <br />For question 10, the correct relationship between standard Gibbs free energy and equilibrium constant is given by the formula:<br /><br />### \(\Delta G^{\circ} = -RT\ln K\)<br /><br />where \(R\) is the gas constant, \(T\) is the temperature in Kelvin, and \(K\) is the equilibrium constant.<br /><br />## Step 4: <br />For question 11, we can use the formula for Gibbs free energy to calculate \(\Delta G^{\circ}\). The formula is:<br /><br />### \(\Delta G^{\circ} = -nFE^{\circ}\)<br /><br />where \(\Delta G^{\circ}\) is the Gibbs free energy, \(n\) is the number of moles of electrons transferred, \(F\) is the Faraday constant (96485 C/mol), and \(E^{\circ}\) is the standard cell potential.<br /><br />## Step 5: <br />For question 12, we can use the Nernst equation to calculate \(E\). The Nernst equation is:<br /><br />### \(E = E^{\circ} - \frac{RT}{nF} \ln Q\)<br /><br />where \(E\) is the cell potential, \(E^{\circ}\) is the standard cell potential, \(R\) is the gas constant, \(T\) is the temperature in Kelvin, \(n\) is the number of moles of electrons transferred, \(F\) is the Faraday constant (96485 C/mol), and \(Q\) is the reaction quotient.
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