Home
Class 12
CHEMISTRY
Standard enthalpy of combustion of cyclo...

Standard enthalpy of combustion of cyclopropane is `-2091 kJ//"mole"` at `25^(@)C` then calculated the enthalpy formation of cyclopropane. If `DeltaH_(f)^(o)(CO_(2))= -393.5 kJ//"mole"` and `Delta H_(f)^(o)(H_(2)O)= -285.8 kJ//"mole"`.

Text Solution

Verified by Experts

The correct Answer is:
53
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    RESONANCE|Exercise exercise-2 Part-3: One or more than type one options correct type|11 Videos

  • THERMODYNAMICS

    RESONANCE|Exercise exercise-2 Part-4 : Comprehension|6 Videos

  • THERMODYNAMICS

    RESONANCE|Exercise Exercise-2 Part-1: Only one option correct type|21 Videos

  • TEST SERIES

    RESONANCE|Exercise CHEMISTRY|50 Videos

Similar Questions

Explore conceptually related problems

The combustion of 1 mol of benzene takes place at 298 K and 1 atm . After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is librated. Calculate the standard entalpy of formation, Delta_(f)H^(Θ) of benzene Given: Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1) Delta_(f)H^(Θ)H_(2)O(l) = -285.83 kJ mol^(-1) .

The standard enthalpy of formation of octane (C_(8)H_(18)) is -250kJ //mol . Calculate the enthalpy of combustion of C_(8)H_(18) . The enthalpy of CO_(2)(g) and H_(2)O(l) are -394 kJ//mol and -286kJ//mol respectively.

Nitroglycerine (MW =227.1) denotes according to the following equation : 2C_(3)H_(5)(NO_(3))_(3)I to 3N_(2)(g)+1//2O_(2)(g)+6CO_(2)(g)+5H_(2)O(g) The standard molar enthalpies of formation, DeltaH_(f)^(@) for the compounds are given bellow: DeltaH_(f)^(@)[C_(3)H_(5)(NO_(3))_(3)]= -364 kJ//mol DeltaH_(f)^(@)[CO_(2)(g)]= -395.5 kJ//mol DeltaH_(f)^(@)[H_(2)O(g)]= -241.8 kJ//mol DeltaH_(f)^(@)[N_(2)(g)]= 0 kJ//mol DeltaH_(f)^(@)[O_(2)(g)]= 0 kJ//mol The enthalpy change when 10g of nitroglycerine is detonated is

Calculate the standard enthalpy of reaction ZnO(s)+CO(g)rarrZn(s)+CO_(2)(g) Given, Delta H_(f)(ZnO,s)=-350KJ//"mole",DeltaH_(f)^(@)(CO_(2),g)= -390KJ//"mole", DeltaH_(f)^(@)(CO,g)=-110KJ//"mole"

Calculate the standard enthalpy of combustion of CH_4 (g) if Delta_f H^(0) (CH_4)=-74.8 Kj mol^(-1) Delta_f H^(0) (CO_2) =- 395 .5 KJ mol^(-1) and Delta f H^(0 ) (H_2 O) =- 285.8 KJ mol^(-1)

The enthalpies of combustion of carbon and carbond monoxide are -393.5 and -283kJ mol^(-1) respectively . The enthalpy of formation of carbond monoxide per mole is :