A chemist designs a galvanic cell that uses these two half-reactions:half-reactionstandard reduction potential2 H₂O(1)+2e→>H2(g)+2 OH (aq)E.ed= -0.83 VredCu²+(aq)+e Cu+ (aq)→>>Answer the following questions about this cell.E° = +0.153 VredWrite a balancedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction thathappens at theanode.Write a balancedequation for the☐☐

Given that :The two half-reactions of the cell are :

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2 H₂O(1)+2e →> H2(g)+2 OH (aq) Cu²+(aq)+e →>> Cu+ (aq) Answer the following questions about this cell. E.ed = -0.83 V red E° = +0.153 V red 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

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2 H₂O(1)+2e →> H2(g)+2 OH (aq) Cu²+(aq)+e →>> Cu+ (aq) Answer the following questions about this cell. E.ed = -0.83 V red E° = +0.153 V red 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

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...

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Draw the galvanic cell from the following half-reactions (use KCl as salt bridge) Al3 + aq + 3rd → Als Ni2 + aq + 2é → Ni (s) Indicates the anode and cathode Indicates where oxidation and reduction occur Indicates the direction of movement of electrons. Indicates the direction of movement of the ions. Write the balanced ionic equation of this equation
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
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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
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Also, What is the E˚value for the electrochemical cell reaction between magnesium and iron?