The standard electrode potential for Daniel cell is 1.1V. Calculate the standard Gibb's energy for the reaction. `Zn_(s)+ Cu_(aq)^(2+) rarr Zn_(aq)^(2+)+Cu_(s)`.

Calculate the equilibrium constant of the reaction: Cu_(s)+2Ag_(aq)^(+) rarr Cu_(aq)^(2+) + 2Ag_(s) , E_^@cell_^@ = 0.46V .

Complete the reaction Zn(s) + NaOH(aq) overset(Delta)rarr

The standard enthalpy of formation of ammonia is -42.19 kJ. Calculate the heat of the following reaction at constant volume. N_2(g) + 3H_2(g) rarr 2NH_3(g)

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: Fe^(2+)(aq) + Ag^+(aq) rarr Fe^(3+)(aq) + Ag(s) . Calculate the Delta_rG and equilibrium constant of the reactions.

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: 2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq) + 3Cd(s) . Also calculate the Delta_rG and equilibrium constant of the reaction.

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: 2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq) + 3Cd(s) Also calculate the DeltarG^@ value of the reaction. (Given: E_(Cr^(3+)//Cr) = -0.74V , E_(Cd^(2+)//Cd) = -0.40V and F =96500C//mol )

The electrode potentials for the two half cell reaction is given below. Determine emf Mg^(2+)+2e^- rarr Mg(s), E=-2.37V Cu^(2+)+2e^- rarr Cu(s), E=+0.34V.

The standard potential of Cu//Cu^(2+) electrodce = -3.34V. It corresponds to the raction

Knowing the equilibrium constant value of a cell reaction at a particular temperature, how will you calculate the standard Gibbs free energy change for the reaction?

Find the energy Q released in this reaction. 1H^2+1H^2 rarr Q+_2He^4