Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Concept explainers
Question
![### 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.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 2 steps with 1 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Write a balanced chemical equation (including states of matter) and a build a cell diagram for an electrochemical cell that has a copper cathode immersed in a solution of Cu2+ ions, and a lead anode immersed in a solution of Pb2+ ions. what is the reaction: ?arrow_forwardA galvanic cell is powered by the following redox reaction: 2+ + 3 Cu²+ (aq) + Cr(OH)3(s) + 5OH¯(aq) → 3 Cut (aq) + Cro (aq) + 4H₂O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 0 E = v V ロ→ロ X 5arrow_forwardI need help with all three questions PLEASE 1) What is the Eldeg cell for the following cell at 294 K? Zn(s) + X2 + (aq) → X(s) + Zn2+ (aq) K = 0.94 x10^4 2) When performing electrolysis of molten NaCl, how many grams of solid sodium are deposited at the cathode when a current of 32.6 A is applied for 1.23 hrs? 3) How many minutes would it take to deposit 4.95 g of Cu(s) from a solution of Cu(NO3)2 when using a current of 35.2 A ?arrow_forward
- Galvanic cell has 2 half reactions O2(g) + 4H+(aq) + 4e- → 2H2O(l) E0red = +1.23 V Cr3+(aq) + 3e- → Cr(s) E0red = -0.74 V Write a balanced equation that describes the cell, ensuring that E0cell > 0 V and Calculate E0cellarrow_forwardG ロ・ロ A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3+ MnO2 (s) + 4H* (aq) +2Cr²* (aq) → Mn²* (aq) + 2H2O (1) +2Cr³+ (aq) Suppose the cell is prepared with 0.190 M H* and 6.41 M Cr²+ in one half-cell and 0.205 M Mn2+ and 1.94 M Cr3+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ☐ ☐ x10 μarrow_forwardIn an electrochemical cell, a metal anode lost 0.286 g while a total volume of 0.04854 L of hydrogen gas was produced. The temperature was 298 K and the barometric pressure was 763.5 mm Hg. At 298 K, the vapor pressure of water is 23.8 mm Hg. What is the molar mass of the metal?arrow_forward
- Both O2 + 2H2O + 4e− → 4OH− and O2(g) + 2H2O (I) → 4OH− (aq)arrow_forward29barrow_forwardSuppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 A£NO3(aq) → Cu(NO,),(aq)+2 Ag(s) E1 E2 sí S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. O-0 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? O DDarrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY