42. Using the following data, calculate the standard standard cell potential for an electrochemical cell based on the reaction below, and tell whether the reaction is spontaneous. 3Fe2+ (aq) + Cr3+ (aq) →Cr (s) + 3Fe³+ (aq) Half-reaction Cr3+ (aq) + 3e →→ Cr (s) Fe2+ (aq) + 2e → Fe (s) Fe3+ (aq) + e → Fe²+ (s) Sn4+ (aq) + 2e Sn²+ (aq) (A) -1.45 V, spontaneous (B) -1.51 V not spontaneous (C) 2.99 spontaneous (D) -1.51 spontaneous (E) -3.05 spontaneous E° (V) -0.74 -0.440 +0.771 +0.154

42. Using the following data, calculate the standard standard cell potential for an electrochemical cell based on the reaction below, and tell whether the reaction is spontaneous. 3Fe2+ (aq) + Cr3+ (aq) →Cr (s) + 3Fe³+ (aq) Half-reaction Cr3+ (aq) + 3e →→ Cr (s) Fe2+ (aq) + 2e → Fe (s) Fe3+ (aq) + e → Fe²+ (s) Sn4+ (aq) + 2e Sn²+ (aq) (A) -1.45 V, spontaneous (B) -1.51 V not spontaneous (C) 2.99 spontaneous (D) -1.51 spontaneous (E) -3.05 spontaneous E° (V) -0.74 -0.440 +0.771 +0.154

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...

See similar textbooks

Similar questions

A 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 5
G 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 μ
An electrochemical cell is based on these two half-reactions: Oxidation: Cu(s) → Cu2+(aq, 0.010 M) + 2 e− Reduction: MnO4 −(aq, 2.0 M) + 4 H+(aq, 1.0 M) + 3 e− → MnO2(s) + 2 H2O(l) Calculate the cell potential.
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Cr(OH)3 (s) +100H¯ (aq) +3Zn²+ (aq) → 2CrO²¯ (aq) +8H₂O (1) + 3 Zn (s) 0 x10 X
A chemist designs a galvanic cell that uses these two half-reactions: 3+ 2+ Fe (aq)+e → Fe (aq) Cro (aq) + 4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is half-reaction spontaneous as written. 0 standard reduction potential Ed=+0.771 V 'red E 'red = -0.13 V ロ→ロ × x10 5
Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- → La (s) E° = -2.37 V Na+ (aq) + e- → Na (s) E° = -2.71 V 1.8 x 10-6 5.7 x 10-18 5.6 x 105 1.7 x 1017
Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag^+(aq)+e^-→Ag(s) What mass of silver plates onto the cathode when a current of 7.9 A flows through the cell for 73 min ?
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu²+ (aq) + e MnO4(aq) + 2 H₂O(1)+3e Cu (aq) → MnO₂(s)+4 OH (aq) standard reduction potential Eº red = 'red = +0.153 V +0.59 V