`H_(2)(g)+1//2O_(2)(g)=H_(2)O(l) , Delta H_(298 K)=-68.32` Kcal. Heat of vapourisation of water at 1 atm and `25^(@)C` is 10.52 Kcal. The standard heat of formation (in Kcal) of 1 mole of water vapour at `25^(@)C` is

H_2(g)+1/2O_2(g)=H_2O(l) , triangleH_298k =-68.32 kcal. Heat of vaporisation of water at 1 atm and 25^@C is 10.52 kcal. The standard heat of formation(in kcal) of 1 mole of water vapour at 25^@C is:

The enthalpy change for chemical reaction is denoted aas DeltaH^(Theta) and DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta) . The relation between enthalpy and internal energy is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal enegry Deltan = change in number of moles, R = gas constant. H_(2)(g) +((1)/(2))O_(2)(g) = H_(2)O(l), DeltaH_(298K) = - 68.00kcal Heat of voporisation of water at 1 atm and 25^(@)C is 10.00 kcal . The standard heat of formation (in kcal) of 1 mole vapour a 25^(@)C is

The enthalpy change for chemical reaction is denoted aas DeltaH^(Theta) and DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta) . The relation between enthalpy and internal enegry is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal enegry Deltan = change in number of moles, R = gas constant. H_(2)(g) +((1)/(2))O_(2)(g) = H_(2)O(l), DeltaH_(298K) = - 68.00kcal Heat of voporisation of water at 1 atm and 25^(@)C is 10.00 kcal . The standard heat of formation (in kcal) of 1 amol vapour a 25^(@)C is

H_(2)(g)+(1)/(2)O_(2)(g)to H_(2)O(l) , Delta H at 298 K = - 285.8 kJ The molar enthalpy of vapourization of water at 1 atm and 25^(@)C is 44 kJ. The standard enthalpy of formation of 1 mole of water vapour at is

H_(2(g)) + 1/2 O_(2(g)) to H_2 O_((l)) , Delta H =- 68 kcal Amount of heat is liberated when 7.2 g of water is decomposed is ______ .

H_(2(g)) + 1/2 O_(2(g)) to H_2 O_((l)) , Delta H =- 68 kcal Amount of heat is liberated when 7.2 g of water is decomposed is ______ .