In the cell reaction Cu(s)+ 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) , E0cell = 0.46 V By doubling the concentration of Cu2+ , E0cell is

Question

In the cell reaction Cu(s)+ 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) , E0cell = 0.46 V By doubling the concentration of Cu2+ , E0cell is (A) doubled (B) halved (C) increased by four times (D) unchanged

Tardigrade Admin · Accepted Answer

We know that, E text cell °= E text cathode °- E text anode ° The equation shows that E text cell ° doesn't depend on the concentration of the ions present in it and hence the value will remain unchanged.

Q. In the cell reaction
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s), E_{ce ll}^{0} = 0.46 V$ By doubling the concentration of $C u^{2 +}, E_{ce ll}^{0}$ is

doubled

halved

increased by four times

unchanged

We know that, $E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ}$
The equation shows that $E_{cell}^{\circ}$ doesn't depend on the concentration of the ions present in it and hence the value will remain unchanged.

Q. In the cell reaction Cu(s)+2Ag+(aq)→Cu2+(aq)+2Ag(s),Ecell0​=0.46V By doubling the concentration of Cu2+,Ecell0​ is