"The Gibbs change (in J) for the given reaction at [Cu2+] = [Sn2+] = 1 M and 298K is : Cu(s) + Sn2+(aq.) $\to$ Cu2+(aq.) + Sn(s); ($E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V$, $E_{C{u^{2 + }}|Cu}^0 = 0.34\,V$) Take F = 96500 C mol–1)"

Question

Accepted Answer

"$\Delta$G = $\Delta$G^o + RTln $\left[ {{{S{n^{ + 2}}} \over {C{u^{ + 2}}}}} \right]$

= –2 × 96500 [(–0.16) – 0.34] + RT$\left[ {{1 \over 1}} \right]$

= 96500 J"

The Gibbs change (in J) for the given reaction at
[Cu²⁺] = [Sn²⁺] = 1 M and 298K is :

Cu(s) + Sn²⁺(aq.) $\to$ Cu²⁺(aq.) + Sn(s);

($E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V$,
$E_{C{u^{2 + }}|Cu}^0 = 0.34\,V$)
Take F = 96500 C mol^–1)

Solution

About this question

Drill 25 more like these. Every day. Free.

The Gibbs change (in J) for the given reaction at [Cu2+] = [Sn2+] = 1 M and 298K is : Cu(s) + Sn2+(aq.) $\to$ Cu2+(aq.) + Sn(s); ($E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V$, $E_{C{u^{2 + }}|Cu}^0 = 0.34\,V$) Take F = 96500 C mol–1)

Solution

About this question

More Electrochemistry questions

Drill 25 more like these. Every day. Free.

The Gibbs change (in J) for the given reaction at
[Cu²⁺] = [Sn²⁺] = 1 M and 298K is :

Cu(s) + Sn²⁺(aq.) $\to$ Cu²⁺(aq.) + Sn(s);

($E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V$,
$E_{C{u^{2 + }}|Cu}^0 = 0.34\,V$)
Take F = 96500 C mol^–1)