The standard enthaply for the reaction `H_(2)(g) + 1//2 O_(2)(g) to H_(2)O(l)` is - 285.76 kJ at 298 K.
Calculate the value of `DeltaH` at 373 K .The molar heat capcities at constant pressure `(C_(P))` in the given temperature range of `H_(2)(g),O_(2)(g) and H_(2)O(l)` are respectively 38.83,16 and `75.312 JK^(-1) mol^(-1)`.

At 1 atm and 298K DeltaH^(0) value of the reaction 2H_(2)(g)+O_(2)(g)to2H_(2)O(l) is -572 kJ. Calculate the change in entropy of the system and surroundings for this reaction. Is this reaction spontaneous at that temperature and pressure? Given: Standard molar entropies of H_(2)(g),O_(2)(g)&H_(2)O(l) at 298K are 130.6, 205.0 and 69.90 J*K^(-1)*mol^(-1) respectively.

H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),DeltaH=-285.8kJ . What will be the value of DeltaH for the reaction: 2H_(2)O(l)to2H_(2)(g) +O_(2)(g) ?

Calculate heat of formation of water at constant volume at 300 K. Given that: H_(2(g))+1/2O_(2(g))rarr H_2O_(l) DeltaH=-284.2kJ

The standard enthalpy of formation of gaseous H_(2)O at 298 K is -241.82 kJ/mol. Calculate DeltaH^(@) at 373 K given the following values of the molar heat capacities at constant pressure : H_(2)O(g)=33.58 " JK"^(-1)" mol"^(-1), " "H_(2)(g)=29.84 " JK"^(-1)" mol"^(-1), " "O_(2)(g)=29.37 " JK"^(-1)" mol"^(-1) Assume that the heat capacities are independent of temperature :