Q1 ## Electrochemistry: Calculating Standard Cell Potential### Task 1:Consider the following half-reactions:- \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \) - Potential: \(-0.76 \, \text{V}\)- \( \text{Cr}^{2+} + 2e^- \rightarrow \text{Cr} \) - Potential: \(-0.91 \, \text{V}\)**Question:** What is the Standard cell potential for the reaction? Options: (a) \( 1.67 \, \text{V} \) (b) \(-1.67 \, \text{V} \) (c) \(-0.15 \, \text{V} \) (d) \( 0.15 \, \text{V} \) ### Explanation:To calculate the standard cell potential, use the formula:\[ E_{\text{cell}} = E_{\text{cathode}} - E_{\text{anode}} \]Consider which half-reaction will act as the cathode and which will act as the anode in order to determine \( E_{\text{cell}} \).

EMF of a cell given by Ecell = Eo(cathode) – Eo(anode) where all are reduction potential. Species…

Answered: 1. Consider the following: Zn²+2e-→ Zn…

1. Consider the following: Zn²+2e-→ Zn -0.76 V Cr²+2e- Cr -0.91 V What is the Standard cell potential for the reaction ? (a) 1.67 V (b) -1.67V (c) -0.15 V (d) 0.15V Calling:

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Question

## Electrochemistry: Calculating Standard Cell Potential

### Task 1:
Consider the following half-reactions:

- \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \)
- Potential: \(-0.76 \, \text{V}\)

- \( \text{Cr}^{2+} + 2e^- \rightarrow \text{Cr} \)
- Potential: \(-0.91 \, \text{V}\)

**Question:**
What is the Standard cell potential for the reaction?
Options:
(a) \( 1.67 \, \text{V} \)
(b) \(-1.67 \, \text{V} \)
(c) \(-0.15 \, \text{V} \)
(d) \( 0.15 \, \text{V} \)

### Explanation:
To calculate the standard cell potential, use the formula:
\[ E_{\text{cell}} = E_{\text{cathode}} - E_{\text{anode}} \]

Consider which half-reaction will act as the cathode and which will act as the anode in order to determine \( E_{\text{cell}} \).

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