Q.A gas mixture of 3.67 lit of ethylene and methane on complete combustion at $25^\circ$C and at 1 atm pressure produce 6.11 lit of carbondioxide. Find out the amount of heat evolved in kJ, during this combustion. ($\Delta H_C(CH_4) = -890$ kJ mol$^{-1}$ and $\Delta H_C(C_2H_4) = -1423$ kJ mol$^{-1}$)

Chemists name a whole family of specific enthalpy changes, each tied to a precisely-defined process. Standard heat of formation $\Delta H_f^0$: enthalpy change forming 1 mole of compound from its elements in standard states (298 K, 1 bar), with every pure element fixed at zero by convention. Standard enthalpy of reaction from formation data: $\Delta H_r^0=\sum\Delta H_f^0(\text{products})-\sum\Delta H_f^0(\text{reactants})$. Heat of combustion $\Delta H_C$: enthalpy change burning 1 mole completely in excess oxygen -- ALWAYS negative, since combustion is always exothermic. Heat of solution: enthalpy change dissolving 1 mole of solute in a specified amount of solvent. Heat of neutralisation: enthalpy change neutralising 1 gram-equivalent of acid by 1 gram-equivalent of base in dilute solution -- remarkably constant at $-57.32$ kJ for ANY strong acid + strong base combination, because Arrhenius's theory says both fully ionise, so the reaction is always really just $H^+(aq)+OH^-(aq)\rightarrow H_2O(l)$ underneath the spectator ions. Molar heat of fusion/vapourisation/sublimation: enthalpy change melting/boiling/sublimi …