63. Calculate the HILL UNUILJ following reaction at 300K. 2CuO , Cu,06 +, Given AH = 145.6 kJ mol-land AS =116.JK-mol- 1) 110.8 kJ mol- 2)221.5 kJ mol- 3) 55.4 kJ moll 4) 145.6 kJ mol

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)

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)

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)

Calculate the temperature at which DeltaG = -5.2 kJ mol^-1, DeltaH = 145.6 kJ mol^-1 and DeltaS = 216 J K^-1 mol^-1 for a chemical reaction

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)

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 at which DeltaG=-5.2 kJ mol^-1 ,DeltaH=145.6kJ mol^-1 and DeltaS=216 JK^-1 mol^-1 for a chemical reaction

Calculate Delta G (in kJ) for the reaction at 300 K, H_(2)(g)+Cl_(2)(g) rarr 2HCl (g) Given at 300 K, BE_(H-H) = 435 kJ mol^(-1), BE_(Cl-Cl) = 240 kJ mol^(-1), BE_(HCl) = 430 kJ mol^(-1) Entropies of H_(2), Cl_(2) and HCl are 131, 223 and 187 JK^(-1) mol^(-1) respectively.

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) .

Calculate the value of DeltaG at 700K for the reaction, nX to mB . Given that value of DeltaH=-113kJ mol^(-1) and DeltaS=-145JK^(-1)mol^(-1).