For the disproportionation reaction
2Cu+(aq) ⇌ Cu(s) + Cu2+(aq) at 298 K. ln K
(where K is the equilibrium constant) is
___________ × 10–1.
Given :
($E_{C{u^{2 + }}/C{u^ + }}^0 = 0.16V$
$E_{C{u^ + }/Cu}^0 = 0.52V$
${{RT} \over F} = 0.025$)
Answer (integer)
144
Solution
$E_{cell}^0$ = $E_{C{u^ + }/Cu}^0$ - $E_{C{u^{2 + }}/C{u^ + }}^0$
<br><br>= 0.52 – 0.16
<br><br>= 0.36 V
<br><br>At equilibrium, E<sub>cell</sub> = 0
<br><br>$E_{cell}^0$ = ${{RT} \over {nF}}$ln K
<br><br>$\Rightarrow$ ln K = ${{E_{cell}^0 \times nF} \over {RT}}$
<br><br>= ${{0.36 \times 1} \over {0.025}}$ = 14.4 = 144 $\times$ 10<sup>-1</sup>
About this question
Subject: Chemistry · Chapter: Electrochemistry · Topic: Electrochemical Cells
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