Enthalpies of formation of CO(g),`CO_2(g),N_2O(g)` and `N_2O_4(g)` are -110,-393,81 and `9.7KJ mol^(-1)` respectively calculate `Delta H_r` for the reaction :`N_2O_4(g)+3CO(g)rarr N_2O(g)+3CO_2(g)`

Enthalpies of formation of CO(g), CO_(2)(g),N_(2)O(g) and N_(2)O_(4)(g) are -110,-393,81 and 9.7kJ*mol^(-1) respectively. Find the value of Delta_(r)H for the reaction: N_(2)O_(4)(g)+3CO(g)toN_(2)O(g)+3CO_(2)(g) .

The enthalpy of formation of CO(g),CO_(2)(g),N_(2)O(g) and N_(2)O_(4)(g) is -110, -393, +811 and 10kJ/mol respectively. for the reaction, N_(2)O_(4)(g)+3CO(g)toN_(2)O(g)+3CO_(2)(g) DeltaH_(r)(kJ//mol) is-

Discuss the rate of the reaction 2N_(2)O_(5(g)) rarr 4NO_(2(g))+O_(2(g))

Delta H- Delta U for the reaction C_3H_8(g) +SO_2 (g) = 3CO_2 (g) + 4H_2O (g) .

The standard heats of formation at 298 K for C CI_4(g) , H_2O (g), CO_2 (g) and HCI (g) are -25.5, -57.8, -94.1 and -22.1 kcal mol^-1 respectively,calculate DeltaH "_(298K)^@ , for the reaction : C Cl_4 (g) + 2H_2O (g) to CO_2 (g) + 4HCI (g)

At 25^(@)C , Delta H^(0) for the reaction , N_(2)(g)+(1)/(2)O_(2)(g) to N_(2)O(g) , is +82 kJ . At this temperature if the standard molar entropies for N_(2)(g),O_(2)(g) and N_(2)O(g) are 191.6, 205.2 and 219.9 J. K^(-1). " mol"^(-1) respectively, calculate Delta S_("univ")^(0) for the reaction.

At 25^(@)C and 1 atm, heat of formation of C_(2)H_(4) (g), CO_(2)(g) and H_(2)O(l) are 52 " kJ mol"^(-1), -394 " kJ mol"^(-1) and -286 " kJ mol"^(-1) respectively. Calculate the heat of combustion of C_(2)H_(4)(g) .

For the equilibrium N_2 (g) + O_2(g) = 2 NO (g)

The heat of reaction for the following reaction (DeltaH^(0)) at 25^(@)C temperatue is -1368 kJ: C_(2)H_(5)OH(l)+3O_(2)(g) to 2CO_(2)(g)+3H_(2)O(l) If the enthalpy of formation of CO_(2)(g) and H_(2)O(l) at 25^(@)C are -393.5 and -285.8 kJ*mol^(-1) respectively, then what will be the value of the standard enthalpy of formation of C_(2)H_(5)OH(l) ?

Write the rate law of 2N_(2)O_(5(g))rarr 4NO_(2(g))+O_(2(g)) reaction.