Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Formation of Nitrogen Oxides from Copper and Nitric Acid
**Context:**
A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides. The following reaction describes the formation of nitrogen monoxide (NO), one of the products.
**Reaction:**
\[ 3\text{Cu}(s) + 8\text{H}^+(aq) + 2\text{NO}_3^-(aq) \longrightarrow 2\text{NO}(g) + 3\text{Cu}^{2+}(aq) + 4\text{H}_2\text{O}(l) \]
**Standard Electrode Potential:**
The standard cell potential (\( E^\circ_{\text{cell}} \)) for this reaction is 0.620 V.
---
**Exercise:**
Calculate the value of the reaction's standard electrode potential (\( E^\circ_{\text{rxn}} \)) at \( 200 \, \text{K} \) given the following conditions:
- \(\text{[H}^+]\) = 0.100 M
- \(\text{[NO}_3^-]\) = 0.0200 M
- \(\text{[Cu}^{2+}]\) = 0.0300 M
- Partial pressure of NO = 0.00300 atm
**Question:**
What is the value of \( E^\circ_{\text{rxn}} \) at these conditions?
\[ E^\circ_{\text{rxn}} \ \boxed{\hspace{3cm}} \text{V} \]
---
**Resources:**
- [See Periodic Table]
- [See Hint]
---
These parameters and conditions are typical for understanding electrochemical cells and the Nernst equation in chemistry. Adjust the values accordingly and employ the Nernst equation to solve for the reaction's standard electrode potential under the provided conditions.](https://content.bartleby.com/qna-images/question/1f1c68a1-c113-41cc-b0cf-42f2666e5687/24919f31-2dae-472b-9344-71c9cdaa8ce5/mzefgt4_processed.png)
Transcribed Image Text:### Formation of Nitrogen Oxides from Copper and Nitric Acid
**Context:**
A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides. The following reaction describes the formation of nitrogen monoxide (NO), one of the products.
**Reaction:**
\[ 3\text{Cu}(s) + 8\text{H}^+(aq) + 2\text{NO}_3^-(aq) \longrightarrow 2\text{NO}(g) + 3\text{Cu}^{2+}(aq) + 4\text{H}_2\text{O}(l) \]
**Standard Electrode Potential:**
The standard cell potential (\( E^\circ_{\text{cell}} \)) for this reaction is 0.620 V.
---
**Exercise:**
Calculate the value of the reaction's standard electrode potential (\( E^\circ_{\text{rxn}} \)) at \( 200 \, \text{K} \) given the following conditions:
- \(\text{[H}^+]\) = 0.100 M
- \(\text{[NO}_3^-]\) = 0.0200 M
- \(\text{[Cu}^{2+}]\) = 0.0300 M
- Partial pressure of NO = 0.00300 atm
**Question:**
What is the value of \( E^\circ_{\text{rxn}} \) at these conditions?
\[ E^\circ_{\text{rxn}} \ \boxed{\hspace{3cm}} \text{V} \]
---
**Resources:**
- [See Periodic Table]
- [See Hint]
---
These parameters and conditions are typical for understanding electrochemical cells and the Nernst equation in chemistry. Adjust the values accordingly and employ the Nernst equation to solve for the reaction's standard electrode potential under the provided conditions.
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