R = 8.314 mol·K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e 2 H20 (1) 1.229 Z2 (s) + 2 e¯ - 3+ A 2z (aq) 0.426 > (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e¯ G2+ H2 (g) + 2 OH¯ (aq) - 0.828 (aq) + 2 e M²+ (aq) + 2 e → G (s) - 1.245 M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. 3+ If the A (aq) solution is diluted to 0.100 M and the G<* (ag) solution is diluted to 0.500 M, what is the initial value of Q under these new conditions? Report your answer with the correct significant figures.

R = 8.314 mol·K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H(aq) + 4 e 2 H20 (1) 1.229 Z2 (s) + 2 e¯ - 3+ A 2z (aq) 0.426 > (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e¯ G2+ H2 (g) + 2 OH¯ (aq) - 0.828 (aq) + 2 e M²+ (aq) + 2 e → G (s) - 1.245 M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. 3+ If the A (aq) solution is diluted to 0.100 M and the G< (ag) solution is diluted to 0.500 M, what is the initial value of Q under these new conditions? Report your answer with the correct significant figures.

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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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

100%

R = 8.314
mol·K
F = 96, 485 moi
AG = AG° + RT · In(Q)
ΔΕΔΕ-().In(Q)
RT
Half Reaction (Note: All given as reduction)
E° (V)
02 (g) + 4 H*(aq) + 4 e
2 H20 (1)
1.229
-
Z2 (s) + 2 e
3+
(aq) + 3 e
2Z (aq)
0.426
→ A (s)
0.292
2 H20 (1) + 2 e
G2+ (aq) + 2 e
H2 (g) + 2 OH (aq)
- 0.828
G (s)
- 1.245
>
M2+ (aq) + 2 e
M (s)
- 1.893
A student constructs a voltaic electrochemical cell with two metal electrodes
[metal G and metal A] in their respective aqueous nitrate solutions
[G(NO3)2 and A(NO3)3].
Use this information, as well as the reduction potentials in the table above to
complete each statement below.
Consider the same cell from the above prompt.
If the A
3+
(aq) solution is diluted to 0.100 M and the G<* (aq) solution is diluted to
2+
0.500 M, what is the initial value of Q under these new conditions?
Report your answer with the correct significant figures.

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