Home
Class 12
CHEMISTRY
The following reaction occurs in a galva...

The following reaction occurs in a galvanic cell `2Cu^+ rarr Cu^(2+) + Cu` If `E_(cu^+ Cu^(2+)) ^@ = +0.16 V and E_(Cu^+Cu)^@` = 0.52 V`, the standard cell potential will be

A

`-1.1 V`

B

`+1.1V`

C

`+0.345 V`

D

`+0.76 V`

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Similar Questions

Explore conceptually related problems

The following redox reaction occurs in a galvanic cell. 2Al_((s))+3Fe_((aq))^(2+)(1M)rarr 2Al_((aq))^(3+)(1M)+3Fe : If E^@anode = -1.66 V and E^@cathode =-0.44 Calculate DeltaG^@ for reaction.

Calculate the standard cell potentials of galvanic cell in which the following reactions take place 2Cr_((s)) + 3Cd_((aq))^(2+)rarr 2Cr_(aq)^(3+) + 3Cd E_(Cr)^@ = -0.740 V, E_(Cd)^@ = -0.403 V, Calculate the Delta_rG^@ and equilibrium constant of the reactions.

The following redox reaction occursin a galvanic cell. 2AI-((s))+3Fe_((aq))(2+)(1M)rarr 2AI_((aq))^(3+)(1M)+3Fe : Calculate E_(Call)^@ if E_(anode)^@=-1.66 V and E_(Sn)^@=-0.136V, E_(Ag)^@=0.799V, (0.8744V)]=-0.44V .

The cell reaction of a cell is Mg+Cu^(2+) to Mg^(2+)+Cu (Given E_(Mg^(2+)//Mg) = -2.37 V , E_(Cu^(2+)//Cu) = 0.337 V ) The e.m.f of the cell will be _________.

Justify the following reactions are redox reaction : CuO(s) + H_2 (g) rarr Cu (s) + H_2O(g)

The equilibrium constant for the reaction in the Daniell call is 1.7xx10^(37) at 25^@C .If E_(Zn^(2+)//Zn)^@=-0.52 , find the standard reduction potential of Cu^(2+)//Cu electrode.

Which of the following alloys contains Cu and Zn ?

The cell reaction of the galvanic cell Cu_((s))|Cu_((aq))^(2+)"||"Hg_((aq))^(2+)|Hg_((l)) is __________.

Calculate standard Gibbs energy change and equilibrium constant at 25^@C for the cell reaction, Cd (s) + Sn^(2o+) (aq) rarr Cd^(2o+) (aq) + Sn (s) Given : E_(Cd)^@ = -0.403V and E_(Sn)^@ = -0.136 V . Write formula of the cell.

Predict whether the following reactions occur under standard state conditions: Oxidation of Ag_((s)) by Cl_(2(g)) E_(Ag)^@ = 0.8V'E_(C12)^@ = 1.36V