Home
Class 12
CHEMISTRY
Write the Nernst equation for the half c...

Write the Nernst equation for the half cell `Zn_((aq))^(2+)//Zn_((s)).`

Text Solution

Verified by Experts

`E_(Zn^(2+)//Zm)=E_(Zn^(2+)//Zn)^(@)-(RT)/(2F)ln [Zn^(2+)]`
Promotional Banner

Similar Questions

Explore conceptually related problems

Write the Nernst equation for Daniel Cell.

Write the cell reaction for the half cell Cl_((aq))^-)//AgCl_((s))Ag.

Write Nernst equation for Daniell cell.

c) Write Nernst equation for the cell represented as: Mg(s)|Mg_((aq))^(+2)||Al_((aq))^(3+)|Al_((S)) .

The emf of the half cell Cu_((aq))^(2+)//Cu_((s)) containing "0.01 M Cu"^(2+) solution is +0.301 V . Calculate the standard emf of the half cell.

Write the Nernst equation and compute the emf of the following cell at 298 K: Sn(s)|Sn^(2+)(0.05M)||H^+(0.02M)|H_2,1atm//Pt

Write the electrochemical cell for the overall cell reaction Zn_((s))+2AgNO_(3)rarr2Ag_((s))+Zn(NO_(3))_(2) .

Write the Nernst equation for an electrode system to calculate standard reduciton potential.

(i) Write the formulation for the galvantic cell in which the reaction Cu(s)+2Ag^+ (aq) toCu^(2+) (aq)+2Ag(s) Takes place . Identify the cathode and anode reactions in it. (ii) Write Nernst eq. and calculate the emf of the following cell. Sn(s)//Sn^(2+)(0.04m)||H^+(0.02M)|H_2(g)|H(s)

Write the nernst equation and calculate the emf of the following cell at 298K. Mg(s)//Mg^(+2)(0.001m)////Cu^(+2)(0.0001M)//Cu(s) Given E^(@)Mg^(+2)//Mg=-2.36V and E^(@)Cu^(+2)//Cu=+0.34 V.