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)`

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)

Estimate the enthalpy of combustion of methane in KJ .mol^(-1) CH_(4)(g)+2O_(2)(g)to CO_(2)(g)+2H_(2)O(g)

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):}

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) b. 4Al(s)+3O_(2)(g) rarr 2Al_(2)O_(3)(s)

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)

Balance the following equations : CH_(4(g))+O_(2(g))toCO_(2(g))+H_(2)O_((g))

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)

Calculate the enthalpy change for the reaction CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) The enethalpy of formation of CH_(4)(g),CO_(2)(g) and H_(2)O(l) are -74.8 kJ mol^(-1) , -393.5 kJ mol^(-1) and -285.8 kJ mol^(-1) respectively.