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).`

The temperature of K at which Delta G =0 for a given reaction with Delta H= -20.5 kJ mol^(-1) and Delta S =- 50.0 JK^(-1)mol^(-1)

For a hypothetical reaction nX to mY , the value of DeltaH =-133 kJ and DeltaS = -145 J K^(-1) . Calcualte the value of DeltaG at 700 K.

The temperature in K at which DeltaG=0 for a given reaction with DeltaH=-20.5 kJ mol^(-1) and DeltaS=-50.0 JK^(-1) mol^(-1) is

For the reaction 2NO(g)+O_(2)(g)to2NO_(2)g Calculate DeltaG at 700K when enthalpy and entropy changes are -113.0kJ" "mol^(-1) and -145J" "K^(-1)mol^(-1) respectively.

For the reaction, 2NO_(g) + O_(2)(g) rarr 2NO_(2)(g) Calculate DeltaG at 700K when enthalpy and entropy changes are -113.0 kJ mol^(-1) and -145 J K^(-1) mol^(-1) , respectively.

For the reaction, 2NO_(g) + O_(2)(g) rarr 2NO_(2)(g) Calculate DeltaG at 700K when enthalpy and entropy changes are -113.0 kJ mol^(-1) and -145 J K^(-1) mol^(-1) , respectively.

The equilibrium constant for the reaction is 10. Calculate the value of DeltaG^(@) , Given R=8.314JK^(-1)"mol"^(-1)T=300K