2 Ag +( aq )+ Cu ( s ) leftharpoons Cu 2+( aq )+2 Ag ( s ) The standard potential E° for this reaction is 0.46 V. Which change will increase the potential the most?

Question

2 Ag +( aq )+ Cu ( s ) leftharpoons Cu 2+( aq )+2 Ag ( s ) The standard potential E° for this reaction is 0.46 V. Which change will increase the potential the most? (A) Doubling the [.Ag+]. (B) Halving the [.Cu2 +]. (C) Doubling the size of the Cu(s) electrode (D) Decreasing the size of the Ag electrode by one-half

Tardigrade Admin · Accepted Answer

E=E° -(0.059/2)log([. C u2 + ]./[. A g+ ].2) The cell potential will increase the most by doubling the concentration of Ag+ ion.

Q. $2 A g^{+} (a q) + C u (s) ⇌ C u^{2 +} (a q) + 2 A g (s)$

The standard potential $E^{\circ}$ for this reaction is 0.46 V. Which change will increase the potential the most?

Doubling the $[A g^{+}]$

Halving the $[C u^{2 +}]$

Doubling the size of the Cu(s) electrode

Decreasing the size of the Ag electrode by one-half

$E = E^{\circ} - \frac{0.059}{2} l o g \frac{[ C u ^{2 +} ]}{[ A g ^{+} ] ^{2}}$

The cell potential will increase the most by doubling the concentration of $A g^{+}$ ion.

Q. 2Ag+(aq)+Cu(s)⇌Cu2+(aq)+2Ag(s) The standard potential E∘ for this reaction is 0.46 V. Which change will increase the potential the most?

Doubling the [Ag+]

Halving the [Cu2+]