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What is the value of the equilibrium constant for this redox reaction? 2Ag+(aq) + Zn (s) → 2Ag (s) + Zn2+(aq) E = +1.56 v K=10(nE∘0.0592) K = 2.25 × 10-26 K = 2.25 × 1026 K = 5.…
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What is the value of the equilibrium constant for this redox reaction? 2Ag+(aq) + Zn (s) → 2Ag (s) + Zn2+(aq) E = +1.56 v K=10(nE∘0.0592) K = 2.25 × 10-26 K = 2.25 × 1026 K = 5.…
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Mar 13, 2019
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What is the value of the equilibrium constant for this redox reaction?
2Ag+(aq) + Zn (s) → 2Ag (s) + Zn2+(aq) E = +1.56 v
K=10(nE∘0.0592)
K = 2.25 × 10-26
K = 2.25 × 1026
K = 5.04 × 10-52
K = 5.04 × 1052
Chemistry
high-school
SUPARNA SOMAN
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D for all the plato homies
Archura
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Mar 14, 2019
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Correct answer: Option D,
K = 5.04 × 10^52
Reason
:
We know that,
Ecell =
,
where n = number of electrons = 2 (in present case)
K = equilibrium constant.
Also, Ecell =
+1.56 v
Therefore, 1.56 =
Therefore, log (K) = 52.703
Therefore, K = 5.04 X 10^52
Martins Balodis
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Mar 20, 2019
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Martins Balodis
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