A solution of nickel chloride (CuC12) was subjected to electrolysis. What is expected to happen? Check all that apply. Refer to the picture below for the reduction potential values of the possible half-reactions: Ni(aq) + 2e → Ni(s) E° = -0.26 V 2H₂001)+2e → H₂(g) + 2OH(aq) E° = -0.83 V 2Cl(aq) → Cl₂(g) + 2e- E° = 1.36 V 2H₂0 (1) → O2(g) + 4H(aq) + 4e¯ E° = 1.23 V a. The metal cathode will be plated with solid nickel. b. Chlorine gas will bubble in the solution. c. Addition of an indicator will make the solution around the cathode appear pink. d. The pH of the solution around the anode will have a pH of less than 7.

A solution of nickel chloride (CuC12) was subjected to electrolysis. What is expected to happen? Check all that apply. Refer to the picture below for the reduction potential values of the possible half-reactions: Ni(aq) + 2e → Ni(s) E° = -0.26 V 2H₂001)+2e → H₂(g) + 2OH(aq) E° = -0.83 V 2Cl(aq) → Cl₂(g) + 2e- E° = 1.36 V 2H₂0 (1) → O2(g) + 4H(aq) + 4e¯ E° = 1.23 V a. The metal cathode will be plated with solid nickel. b. Chlorine gas will bubble in the solution. c. Addition of an indicator will make the solution around the cathode appear pink. d. The pH of the solution around the anode will have a pH of less than 7.

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

Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Ni Ag 1.0 M Ni2+ 1.0 M Ag* The standard reduction potentials are as follow: Ni2+ + 2 e- → Ni(s), E° = -0.25 Ag* + e - Ag(s), E° = 0.7996 When current is allowed to flow, which species is oxidised? Select one: а. Ag b. Cannot be determined from the data given. C. Ni2+ O d. Ag* O e. Ni
Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: Ni?+ (aq) + Cd(s) → Ni(s) + Cd²+ (aq) Answer: kJ K for this reaction would be than one.
O ELECTROCHEMISTRY Analyzing a galvanic cell A galvanic cell is powered by the following redox reaction: 3 Br₂(1) + 2 Cr(OH)3(s) + 10OH (aq) - → 6 Br (aq) + 2 CrO (aq) + 8 H₂0(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 E = OV ローロ é X Do ?
Use standard reduction potentials to find the equilibrium constant for the following reaction at 25°C: Mg?*(aq) + Pb(s) =Mg(s) + Pb2+(aq) Enter your answer in scientific notation to one significant digit. K = × 10
please step by step solution.
Examine the following half-reactions and select the strongest reducing agent among the species listed. AuBr4(aq) + 3e– → Au(s) + 4Br–(aq) E° = 0.854 V Mn2+(aq) + 2e– → Mn(s) E° = –1.185 V K+(aq) + e– → K(s) E° = –2.931 V F2O(aq) + 2H+(aq) + 4e– → 2F–(aq) + H2O(l) E° = 2.153 V Group of answer choices K K+ F2O F–
29b
Based on standard reduction potentials (in second table below), will each of these reactions (in table 1) take place? How to calculate this?
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu²+ (aq) + Pb(s) → Cu(s) + Pb²+ (aq) 2+ Cu²+ (aq) + 2e Pb²+ (aq) + 2e → Cu(s) Fre 0.337 V → Pb(s) Fe -0.126 V red = Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be | than zero.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction + 21O3(aq)+ 12 H¹ (aq)+10e¯ Cl₂(g) +2e 1₂(s) + 6H₂O(1) → 2 C1 (aq) standard reduction potential E=+1.195 V 'red E 70 = +1.359 V red
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy delta G^0 for the following redox reaction. I2(s) + 6H2O(l) + 5 Cl2(g) -> 2IO3-(aq) + 12H+(aq) + 10Cl-(aq)Be sure your answer has the correct number of significant digits.
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Cu²+ (aq) + 2Cu+ (aq) → Cu(s) + 2Cu²+ (aq) 2+ Cu²+ (aq) + 2e → Cu(s) Ee = 0.337 V red 0.153 V = 2+ Cu²+ (aq) +e → Cut (aq) E red AG° kJ K for this reaction would be than one.