Calculate the change in enthalpy ,`DeltaH`, for the combustion of 11.2 L of hydrogen gas , measured at `0^(@)C` and 1 atm pressure , to orm `H_(@)O(g)`:
`{:(DeltaH_(f)^(@),(KJ.mol^(-1))),(H_(2)O(g),-241.8):}`

Calculate the ethalpy of combustion of ethylene (g) to form CO_(2) (gas) and H_(2)O (gas) at 298 K and 1 atmospheric pressure. The enthalpies of formation of CO_(2),H_(2)O and C_(2)H_(4) are -393.7, -241.8+52.3 kJ per mole respectively.

Calculate the ethalpy of combustion of ethylene (g) to form CO_(2) (gas) and H_(2)O (gas) at 298 K and 1 atmospheric pressure. The enthalpies of formation of CO_(2),H_(2)O and C_(2)H_(4) are -393.7, -241.8+52.3 kJ per mole respectively.

Calculate the standard enthalpy of formation of acetylena from the following data: C(s)+O_(2)(g)to CO_(2)(g), DeltaH^(@)=-393.5KJmol^(-1) H_(2)(g)+(1)/(2)O_(2)(g)to H_(2)O(l),DeltaH^(@)=-285 .8KJmol^(-1) 2C_(2)H_(2)(g)+50_(2)(g)to 4Co_(2)(g)+2H_(2)O(l0, DeltaH^(@)=-2598.8KJmol^(-1)

Calculate DeltaH^(@) for the reaction : TiCl_(4)(g)+2H_(2)O(l)to TiO_(2)(s)+4Hcl(g) {:(DeltaH_(f)^(@),(KJ.mol,^(-1))),(TiCl_(4)(g),-763),(H_(2)O(l),-286),(TiO_(2)(s),-945),(HCl(g),-92):}

Calculate the enthalpy of formation of Delta_(f)H for C_(2)H_(5)OH from tabulated data and its heat of combustion as represented by the following equaitons: i. H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g), DeltaH^(Theta) =- 241.8 kJ mol^(-1) ii. C(s) +O_(2)(g) rarr CO_(2)(g),DeltaH^(Theta) =- 393.5kJ mol^(-1) iii. C_(2)H_(5)OH (l) +3O_(2)(g) rarr 3H_(2)O(g) + 2CO_(2)(g), DeltaH^(Theta) =- 1234.7kJ mol^(-1) a. -2747.1 kJ mol^(-1) b. -277.7 kJ mol^(-1) c. 277.7 kJ mol^(-1) d. 2747.1 kJ mol^(-1)