### Electrochemical Cell Analysis at 25°C1. **For the following electrochemical cell at 25°C:** \[ \text{Fe}_{(s)} \;|\; \text{Fe}^{2+}_{(aq)} \;\|\; \text{H}^+_{(aq)} \;|\; \text{Pt, H}_2_{(g)} \;(\text{P} = 1.00 \; \text{atm}) \] a. **Write the half-reaction at the anode.** \[ \text{Fe}_{(s)} \rightarrow \text{Fe}^{2+}_{(aq)} + 2\text{e}^- \] b. **Write the half-reaction at the cathode.** \[ 2\text{H}^+_{(aq)} + 2\text{e}^- \rightarrow \text{H}_2_{(g)} \] c. **Write the overall redox reaction.** \[ \text{Fe}_{(s)} + 2\text{H}^+_{(aq)} \rightarrow \text{Fe}^{2+}_{(aq)} + \text{H}_2_{(g)} \] d. **Calculate \(\Delta G^\circ\) in kJ** *(Solution required)* e. **Calculate \(E_{\text{cell}}\) for \([\text{H}^+]\) = 0.10 M and \([\text{Fe}^{2+}]\) = 0.50 M** *(Solution required)* f. **Calculate \(K\) at 25°C** *(Solution required)*This section examines the electrochemical processes occurring in a galvanic cell, detailing half-reactions and asking for thermodynamic and equilibrium calculations based on concentration and pressure conditions.

1. For the following electrochemical cell at 25°C: Fe(s) Fe (aq) ||H(aq) | Pt, H₂(g) (P=1.00 atm) a. Write the half reaction at the anode. Fe(s) Fag) + Zes H₂(g) b. Write the half reaction at the cathode. Haze c. Write the overall redox reaction. Fe(s)+2HFeaq) + H₂ (g) d. calculate AG in kJ e. calculate Ecell for [H*] = 0.10 M and [Fe²+] = 0.50 M f. calculate K at 25°C

1. For the following electrochemical cell at 25°C: Fe(s) Fe (aq) ||H(aq) | Pt, H₂(g) (P=1.00 atm) a. Write the half reaction at the anode. Fe(s) Fag) + Zes H₂(g) b. Write the half reaction at the cathode. Haze c. Write the overall redox reaction. Fe(s)+2HFeaq) + H₂ (g) d. calculate AG in kJ e. calculate Ecell for [H*] = 0.10 M and [Fe²+] = 0.50 M f. calculate K at 25°C

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

### Electrochemical Cell Analysis at 25°C

1. **For the following electrochemical cell at 25°C:**

\[ \text{Fe}_{(s)} \;|\; \text{Fe}^{2+}_{(aq)} \;\|\; \text{H}^+_{(aq)} \;|\; \text{Pt, H}_2_{(g)} \;(\text{P} = 1.00 \; \text{atm}) \]

a. **Write the half-reaction at the anode.**

\[ \text{Fe}_{(s)} \rightarrow \text{Fe}^{2+}_{(aq)} + 2\text{e}^- \]

b. **Write the half-reaction at the cathode.**

\[ 2\text{H}^+_{(aq)} + 2\text{e}^- \rightarrow \text{H}_2_{(g)} \]

c. **Write the overall redox reaction.**

\[ \text{Fe}_{(s)} + 2\text{H}^+_{(aq)} \rightarrow \text{Fe}^{2+}_{(aq)} + \text{H}_2_{(g)} \]

d. **Calculate \(\Delta G^\circ\) in kJ**

*(Solution required)*

e. **Calculate \(E_{\text{cell}}\) for \([\text{H}^+]\) = 0.10 M and \([\text{Fe}^{2+}]\) = 0.50 M**

*(Solution required)*

f. **Calculate \(K\) at 25°C**

*(Solution required)*

This section examines the electrochemical processes occurring in a galvanic cell, detailing half-reactions and asking for thermodynamic and equilibrium calculations based on concentration and pressure conditions.

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