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.

a) Explain the effect of temperature on the spontaneity of a process based on Gibbs equation. b) For a reaction 2A(g)+B(g)rightarrow2D(g) , enthalpy and entropy changes are - 20.5 kJ mol^-1 and -50.4 J K^-1mol^-1 respectively. Predict whether the reaction occurs at 25^oC.

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).

DeltaH for the reaction at 298 K CO(g)+1//2O_(2)(g) is 282.85 KJ mol^(-1) . Calculate DeltaU of the reaction.

DeltaH for the reaction at 298 K CO(g)+1//2O_(2)(g) is 282.85 KJ mol^(-1) . Calculate DeltaU of the reaction.