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.

Equilibrium constant of the reaction, 2Cu^(o+)(aq)rarr Cu^(2o+) (aq) + Cu_((s)) is 1.2 xx 10^6 . What is the standard potential of the cell in which the reaction takes place?

Calculate equilibrium constant for the reaction, Ni_((s)) + 2Ag_((aq))^(2+) rarr Ni_((aq))^(2+) + 2Ag_((s)) at 25^@C E_(Ni)^@ =- 0.25V and E_(Ag)^@ = 0.799V .

The equilibrium constant for the following reactio is 1.6 xx 10^5 at 1024 K. H_2(g) + Br_2(g) hArr 2HBr(g) Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

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 mixture of 1.57 mol of n_2 ,1.92 mol of H_2 and 8.13 mol of NH_3 is introduced into a 20 L reaction vessel at 500 kAt this temperature,the equilibrium constant. K_C for the reaction N_2(g) + 3H_2(g) hArr 2NH_3(g) is 1.7 xx 10 ^2 .Is the reaction mixture at equilibrium?If not,what is the direction of the net reaction?

Equilibrium constant of the reaction, 2Cu^(o+)(aq)rarr Cu^(2o+)(aq) + Cu(s) is 1.2xx 10^6 . What is the standard potential of the cell in which the reaction takes place ?

The equilibrium constant (K_c) for the reaction N_2(g) + O_2 (g) rarr 2NO (g) at temperature T is 4xx10^(-4) .The value of K_c for the reaction, NO(g) rarr1//2 N_2 (g) +1//2O_2 (g) at the same temperature is:

The equilibrium constant for the following reaction at 25^@C is 2.9 xx 10^9 . Calculate standard voltage of the cell. Cl_(2(g)) +Br_(aq)^- narr Br(2(i))+2CI_((aq))^- .

The rate constant of a reaction is 2.1 xx 10^(-2) litre mol^(-1)s^(-1) . The order of reaction is

The rate constant for a first order reaction is 7.0xx10^(-4) s^(-1) . If initial concentration of reactant is 0.080 M, what is the half life of reaction ?