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Please write the value for their electrode potential: Predict the products of electrolysis of the following and write the anode reaction, the cathode reaction and the overall reaction. AGNO3(a9)\ You may refer to the following values of standard reduction potentials + 4H* (aq) + 3 e- → NO(g) + 2 H2O1) NO: (aq) E° = +0.956 V 3Ag6) 2 H2Oa) + 2 e- → H2g)+2 OH (aq) → Na(s) → K(s) Ag"(aq) + e- E° = +0.800 V E° = – 0.42 V Na* (ag) + e → E° =– 2.71 V '(aq) + e- E° = – 2.93 V

Please write the value for their electrode potential: Predict the products of electrolysis of the following and write the anode reaction, the cathode reaction and the overall reaction. AGNO3(a9)\ You may refer to the following values of standard reduction potentials + 4H* (aq) + 3 e- → NO(g) + 2 H2O1) NO: (aq) E° = +0.956 V 3Ag6) 2 H2Oa) + 2 e- → H2g)+2 OH (aq) → Na(s) → K(s) Ag"(aq) + e- E° = +0.800 V E° = – 0.42 V Na* (ag) + e → E° =– 2.71 V '(aq) + e- E° = – 2.93 V

Chemistry
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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Please write the value for their electrode potential: Predict the products of electrolysis of the following and write the anode reaction, the cathode reaction and the overall reaction. AGNO3(a9)\ You may refer to the following values of standard reduction potentials + 4H* (aq) + 3 e- → NO(g) + 2 H2O1) NO: (aq) E° = +0.956 V 3Ag6) 2 H2Oa) + 2 e- → H2g)+2 OH (aq) → Na(s) → K(s) Ag"(aq) + e- E° = +0.800 V E° = – 0.42 V Na* (ag) + e → E° =– 2.71 V '(aq) + e- E° = – 2.93 V
Transcribed Image Text:Please write the value for their electrode potential: Predict the products of electrolysis of the following and write the anode reaction, the cathode reaction and the overall reaction. AGNO3(a9)\ You may refer to the following values of standard reduction potentials + 4H* (aq) + 3 e- → NO(g) + 2 H2O1) NO: (aq) E° = +0.956 V 3Ag6) 2 H2Oa) + 2 e- → H2g)+2 OH (aq) → Na(s) → K(s) Ag"(aq) + e- E° = +0.800 V E° = – 0.42 V Na* (ag) + e → E° =– 2.71 V '(aq) + e- E° = – 2.93 V
2.) AGNO3 (ag) - Ag+ and NO,- o Possible Reduction(Cathode) Half-Reaction: E° = Ag (s) Ag + e → (aq) E° = 2H200 + 2e- → + 20H (aq) H2 (g) => /Which half reaction will take place at cathode/ o Possible Oxidation(Anode) Half-Reaction: E° = E° = => /Which half reaction will take place at anode/ HALF-REACTION: Cathode(Reduction): Anode(Oxidation): Overall: The product produced at cathode: REASON: • The product produced at anode: REASON:
Transcribed Image Text:2.) AGNO3 (ag) - Ag+ and NO,- o Possible Reduction(Cathode) Half-Reaction: E° = Ag (s) Ag + e → (aq) E° = 2H200 + 2e- → + 20H (aq) H2 (g) => /Which half reaction will take place at cathode/ o Possible Oxidation(Anode) Half-Reaction: E° = E° = => /Which half reaction will take place at anode/ HALF-REACTION: Cathode(Reduction): Anode(Oxidation): Overall: The product produced at cathode: REASON: • The product produced at anode: REASON:
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