1. Tardigrade
  2. Question
  3. Chemistry
  4. In the cell reaction Cu(s)+ 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) , E0cell = 0.46 V By doubling the concentration of Cu2+ , E0cell is

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Q. In the cell reaction
$Cu(s)+ 2Ag^{+} (aq) \to Cu^{2+} (aq) + 2Ag(s) , E^{0}_{cell} = 0.46 \, V$ By doubling the concentration of $Cu^{2+} , E^{0}_{cell}$ is

BITSATBITSAT 2014

Solution:

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