In the reaction `2H_(2)(g) + O_(2)(g) rarr 2H_(2)O (l), " "Delta H = - xkJ`

The enthalpy of reaction for the reaction 2H_(2) (g) + O_(2) (g) rarr 2H_(2) O (l) " is " Delta_(r) H^(Θ) = - 572 kJ mol^(-1) What will be standard enthalpy of formation of H_(2) O (l) ?

For the reaction : H_(2)(g) + (1)/(2)O_(2)(g) rarr H_(2)O(l), Delta H = - 68 kcalmol^(-1) The heat change for the decomposition of 7.2 g of water is

For the reaction 2H_(2(g)) + o_(2(g)) rarr 2H_(2)O_((g)), Delta H^(@) = - 573.2 kJ . The heat of decomposition of water per mol is:

For the thermochemical equation, 2H_(2(g)) + O_(2(g)) rarr 2H_(2)O_(l) , Delta H = - 571.6 kJ Heat of decomposition of water is :

Calculate in kJ for the following reaction : C(g) + O_(2)(g) rarr CO_(2)(g) Given that, H_(2)O(g) + C(g) + H_(2)(g) , Delta H = +131 kJ CO(g) + 1/2 O_(2)(g) rarr CO_(2)(g), " " Delta H = -242 kJ H_(2)(g) + 1/2 O_(2)(g) rarr H_(2)O(g), " "DeltaH = -242 kJ

Calculate in kJ for the following reaction : C(g) + O_(2)(g) rarr CO_(2)(g) Given that, H_(2)O(g) + C(g) + H_(2)(g) , Delta H = +131 kJ CO(g) + 1/2 O_(2)(g) rarr CO_(2)(g), " " Delta H = -242 kJ H_(2)(g) + 1/2 O_(2)(g) rarr H_(2)O(g), " "DeltaH = -242 kJ

Calculate DeltaG_(298)^(@) and DeltaS_(298)^(@) for the reaction : 2H_(2(g))+O_(2(g)) rarr 2H_(2)O_((l)): DeltaH_(298)^(@) = -136.64kcal . Given that O_(2(g))+4H^(+)+4e rarr 2H_(2)O_((l)), E^(@) = 1.23V 2H_(2(g)) rarr 4H^(+)+4e, E^(@) = 0.00V