Calculate the temperature, at which the reaction given below is at equilibrium,
`Ag_(2)O(s) to 1/2 O_(2)(g)`
Given, `DeltaH = 30.5 kJ mol^(-1)` and `DeltaS = 0.066 kJK^(-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)

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)

The temperature at which the reaction, Ag_(2)O(s)rarr2Ag(s)+1//2O_(2)(g) Is at equilibrium is ..., Given DeltaH=30.5KJ mol^(-1) and DeltaS =0.066KJK^(-1)

The temperature at which the reaction, Ag_(2)O(s)rarr2Ag(s)+1//2O_(2)(g) Is at equilibrium is ..., Given DeltaH=30.5KJ mol^(-1) and DeltaS =0.066KJK^(-1)

The temperature at which the reaction : Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) is at equilibrium is …….., Given Delta H=30.5 KJ mol^(-1) and Delta S = 0.5 KJ mol^(-1) :

The temperature at which the reaction, Ag_2O(s)rarr2Ag(s)+I//2O_2(g) is at equilibrium is…….., Given triangleH =30.5 kJ mol^-1 and triangle S =0.066 kJ 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)

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)

Assume DeltaH^(@) and DeltaS^(@) to be independent of temperature, at what temperature with the reaction given below becomes spontaneous? N_(2)(g) + O_(2)(g) to 2NO(g) DeltaH^(@) = 180.8 kJ mol^(-1)