Free energy change at 300k for following reaction will be `2CuO(s) to CuO(s)+0.5 O_2 (g)`
given that `Delta`H=145.6KJ `mol^(-1)` and `Delta`S=116J`K^(-1) mol^(-1)`

Calculate the free energy change for the following reaction at 300 K. 2CuO_((s)) rarr Cu_(2)O_((s))+(1)/(2)O_(2(g)) Given Delta H = 145.6 kJ mol^(-1) and Delta S = 116.JK^(-1) mol^(-1)

Predict whether the following reaction is possible or not at 300k . 2CuO(s) rarr Cu_(2)O(s) +1//2O_(2)(g) DeltaH =- 144.6 kJ mol^(-1), DeltaS = 0.116 kJ mol^(-1)

Calculate the temperature above which the reaction of lead oxide to lead in the following reaction become spontaneous. PbO(s) + C(s) rarr Pb(s) + CO(g) Given Delta H = 108.4 kJ mol^(-1), Delta S = 190 JK^(-1) mol^(-1)

Calculate the standard free energy change for the following reaction at 27^@C . H_2(g) + I_2(g) to 2HI(g) , DeltaH^@ = + 51.9 kJ [Given : DeltaS_(H_2)^@ = 130.6 JK^(-1) mol^(-1) DeltaS_(I_2)^@ = 116.7 JK^(-1) mol^(-1) DeltaS_(HI)^@ = 206.3 JK^(-1) mol^(-1)] . Predict whether the reaction is feasible at 27°C or not.

Calculate the temperature above which the reduction of lead oxide to lead in the following reaction become spontaneous. PbO(s) + C(s) rightarrow Pb(s) + CO(g) Given Delta H = 118.4 kJ mol^(-1), Delta S = 200 JK^(-1) mol^(-1) .

Calculate the standard free energy change for the following reaction Zn(s) + Cu^(2+)(aq) to Zn^(2+) (aq) + Cu(s) Given : Delta_fG^@ [Cu^(2+)(aq)] = 65.0kJ mol^(-1) Delta_f G^@ [ Zn^(2+) (aq)] = -147.2 kJ mol^(-1)

Calculate the value of equilibrium constant, K for the following reaction at 400 K. 2NOCl(g) hArr 2NO (g) + Cl_2(g) DeltaH^@ = 80.0 kJ mol^(-1), DeltaS^@ = 120 KJ^(-1) mol^(-1) at 400 K, R = 8.31 JK^(-1) mol^(-1) .

The temperature at which the given reaction is at equilibrium Ag_(2)O_(s) rightarrow 2Ag(s) + 1/2 O_(2)(g) Delta H = 40.5 kJ mol^(-1) and DeltaS= 0.086 k J mol^(-1) K^(-1)

Calculate the equilibrium constant for the following reaction at 298 K: 2H_2O (l) to 2H_2(g) + O_2(g) Given : Delta_fG^@ [ H_2O (l)] = - 273.2 kJ mol^(-1) R = 8.314 J mol^(-1) K^(-1) .

Calculate the change in entropy for the following reaction 2CO(g) +O_(2)(g) rarr 2CO_(2)(g) Given: S_(CO)^(Theta)(g)=197.6 J K^(-1)mol^(-1) S_(O_(2))^(Theta)(g)=205.03 J K^(-1)mol^(-1) S_(CO_(2))^(Theta)(g)=213.6 J K^(-1)mol^(-1)