At `298K`, the enthalpy of combustion of `CH_(4)` corresponds to the reaction
`CH_(4)(g) +2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(g)`

For the first order reaction 2N_(2)O_(5)(g) rarr 4NO_(2)(g) + O_(2)(g)

Calculate the standard enthalpy of formation of CH_(3)OH(l) from the following data: CH_(3)OH(l)+3/2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(l), …(i), Delta_(r)H_(1)^(Θ)=-726 kJ mol^(-1) C(g)+O_(2)(g) rarr CO_(2)(g), …(ii), Delta_(c )H_(2)^(Θ)=-393 kJ mol^(-1) H_(2)(g)+1/2O_(2)(g) rarr H_(2)O(l), ...(iii), Delta_(f)H_(3)^(Θ)=-286 kJ mol^(-1)

For the reaction CO_((g)) + (1)/(2) O_(2(g)) to CO_(2(g)) K_(p)//K_(c) is

Diborane isa potential rocket fuel that undergoes combustion according to the reaction, B_(2)H_(6)(g) +3O_(2)(g) rarr B_(2)O_(3)(g) +3H_(2)O(g) From the following data, calculate the enthalpy change for the combustion of diborane:

Diborane is a potential rocket fuel that undergoes combustion according to the reaction, B_(2)H_(6)(g) +3O_(2)(g) rarr B_(2)O_(3)(g) +3H_(2)O(g) From the following data, calculate the enthalpy change for the combustion of diborane:

Compute the standard free enegry of the reaction at 27^(@)C for the combustion fo methane using the give data: CH_(4)(g) +2O_(2)(g) rarr CO_(2)(g) +2H_(2)O(l) {:(Species,CH_(4),O_(2),CO_(2),2H_(2)O(l)),(Delta_(f)H^(Theta)(kJmol^(-1)),-74.8,-,-393.5,-285.8),(S^(Theta)(JK^(-1)mol^(-1)),186,205,214,70):}

Calculate the enthalpy of formation of acetic acid from the following data. CH_(3)COOH(l)+2O_(2)(g)rarr 2CO_(2)(g)+2H_(2)O(l), " " Delta H=-207.9 k cal

Use the standard enthalpies of formation and calculation the enthalpy changes accompanying the following reaction: a. CH_(4)(g)+2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(l) Given, enthalpies of formation of CH_(4) ,CO_(2) and H_(2)O are 74.8 kJmol^(-1) ,−393.5 kJmol^(−1) ,−286 kJmol^(−1) respectively.

Standard heat of formation of CH_(4)(g), CO_(2)(g) and H_(2)O(l) are -75, -393.5, -286 kJ respectively. Find out the change in enthalpy for the reaction. CH_(4)(g)+2O_(2)(g)rarr CO_(2)(g)+2H_(2)O(l)

Reaction of methanol with dioxygen was carried out and DeltaU was found to be -726"kJ mol"^(-1) at 298 K. The enthalpy change for the reaction will be CH_(3)OH_((l))+(3)/(2)O_(2(g)) rarr CO_(2(g))+2H_(2)O_((l)) , DeltaH=-726"kJ mol"^(-1)