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Question

(A) The cell reaction is: $Al_{(s)} + 3Ag^{+}_{(aq)} 	o Al^{3+}_{(aq)} + 3Ag_{(s)}$The number of electrons transferred $(n)$ is $3$.The Nernst equati

Vedclass · Accepted Answer

$1.5496$

Vedclass · Answer

(A) The cell reaction is: $Al_{(s)} + 3Ag^{+}_{(aq)} 	o Al^{3+}_{(aq)} + 3Ag_{(s)}$The number of electrons transferred $(n)$ is $3$.The Nernst equation is given by: $E_{cell} = E^o_{cell} - \frac{0.06}{n} \log \frac{[Al^{3+}]}{[Ag^{+}]^3}$Substituting the given values: $1.50 = E^o_{cell} - \frac{0.06}{3} \log \frac{0.30}{(0.10)^3}$$1.50 = E^o_{cell} - 0.02 \log \frac{0.30}{0.001}$$1.50 = E^o_{cell} - 0.02 \log (300)$$1.50 = E^o_{cell} - 0.02 (\log 3 + \log 100)$$1.50 = E^o_{cell} - 0.02 (0.48 + 2)$$1.50 = E^o_{cell} - 0.02 (2.48)$$1.50 = E^o_{cell} - 0.0496$$E^o_{cell} = 1.50 + 0.0496 = 1.5496 \, V$

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