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. Fis) b. Write the half reaction at the cathode Haze c. Write the overall redox reaction. Fe(s)+H→ d. calculate ÄGº in kJ AG=AH-TAS treo > H₂(g) Felaq) + Hz (g) f. calculate K at 25°C Felag) e. calculate Ecal for [H] = 0.10 M and [Fe²] = 0.50 M Ecell = Ereduced - Eoxidized
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. Fis) b. Write the half reaction at the cathode Haze c. Write the overall redox reaction. Fe(s)+H→ d. calculate ÄGº in kJ AG=AH-TAS treo > H₂(g) Felaq) + Hz (g) f. calculate K at 25°C Felag) e. calculate Ecal for [H] = 0.10 M and [Fe²] = 0.50 M Ecell = Ereduced - Eoxidized
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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Parts D, E, & F I'm stuck on.
![For the following electrochemical cell at 25°C:
\[ \text{Fe}(s) | \text{Fe}^{2+}(aq) || \text{H}^+(aq) | \text{Pt}, \text{H}_2(g) \, (P = 1.00 \, atm) \]
a. **Write the half reaction at the anode.**
\[ \text{Fe}(s) \rightarrow \text{Fe}^{2+}(aq) + 2e^- \]
b. **Write the half reaction at the cathode.**
\[ 2\text{H}^+(aq) + 2e^- \rightarrow \text{H}_2(g) \]
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.**
\[ \Delta G = \Delta H - T \Delta S \]
e. **Calculate \( E_{\text{cell}} \) for \([\text{H}^+] = 0.10 \, \text{M and} \, [\text{Fe}^{2+}] = 0.50 \, \text{M}\).**
\[ E_{\text{cell}} = E_{\text{reduced}} - E_{\text{oxidized}} \]
f. **Calculate K at 25°C.**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb7f6f8cc-4a1c-4f0d-863a-df6012bc4cc8%2Fb923f410-a3dd-4eaf-8d91-66786a86901f%2Fyjfyvm9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:For the following electrochemical cell at 25°C:
\[ \text{Fe}(s) | \text{Fe}^{2+}(aq) || \text{H}^+(aq) | \text{Pt}, \text{H}_2(g) \, (P = 1.00 \, atm) \]
a. **Write the half reaction at the anode.**
\[ \text{Fe}(s) \rightarrow \text{Fe}^{2+}(aq) + 2e^- \]
b. **Write the half reaction at the cathode.**
\[ 2\text{H}^+(aq) + 2e^- \rightarrow \text{H}_2(g) \]
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.**
\[ \Delta G = \Delta H - T \Delta S \]
e. **Calculate \( E_{\text{cell}} \) for \([\text{H}^+] = 0.10 \, \text{M and} \, [\text{Fe}^{2+}] = 0.50 \, \text{M}\).**
\[ E_{\text{cell}} = E_{\text{reduced}} - E_{\text{oxidized}} \]
f. **Calculate K at 25°C.**
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