Home
Class 12
CHEMISTRY
The standard enthalpy of for ation (Delt...

The standard enthalpy of for ation `(Delta_(f) H^(@))` at 298 K for methane, `C H _(4) (g)` , is `-74 . 8 KJ mol^(-1)`.The additional information required to determine the average energy for C-H bond formation would be

A

the dissociation energy of `H_(2)` and enthalpy fo sublimation of carbon

B

latent heat of vapourisation of methane

C

the first four ionization energies of carbon and electron gain enthalpy of hydrogen

D

the dissociation energy of hydrogen molecule , `H_(2)`

Text Solution

Verified by Experts

The correct Answer is:
A
`C=2H_(2) rarr CH_(4), DeltaH^(@) = -74.8 KJ mol^(-1)`
In order to calculate average energy for C-H bond formation we should know the following data. `C("graphite") rarr C(g), DeltaH, `=enthalpy of sublimation of carbon
`H_(2)(g) rarr 2H(g) , DeltaH^(@)` bond dissociation energy of `H_(2)`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise exercise-3 Part-3 :(Subjective questions)|6 Videos

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise exercise-3 Part-3 :(Subjective questions)Section A|1 Videos

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise exercise-3 Part-1 :(previous years)|8 Videos

  • TEST SERIES

    RESONANCE ENGLISH|Exercise CHEMISTRY|50 Videos

Similar Questions

Explore conceptually related problems

The standard enthalpy of formation (Delta_(f)H^(@)) at 298K for methane (CH_(4(g))) is -74.8kJ mol^(-1) . The additional information required to determine the average energy for C-H bond formation would be :

The standard enthalpy of formation of NH3 is -46.0 kJ mol^(-1) . If the enthalpy of formation of H_2 from its atoms is -436 kJ mol and that of N_2 is -712 kJ mol, the average bond enthalpy of N - H bond in NH_3 is

The enthalpy of atomisation for the reaction CH_(4) (g) rarr C (g) + 4H (g) " is " 1665 kJ mol^(-1) . What is the bond energy of C - H bond ?

The enthalpy change (DeltaH) for the process, N_(2)H_(4)(g)to 2N(g)+4H(g) is is 1724 kJ mol^(-1) . If the bond energy of N-H bond in ammonia is 391 kJ mol^(-1) , what is the bond energy for N-N bond in N_(2)H_(4) ?

Bond dissociation enthalpies of H_(2(g)) and N_(2(g)) are "426.0 kJ mol"^(-1) and "941.8 kJ mol"^(-1) , respectively, and enthalpy of formation of NH_(3(g))" is "-"46 kJ mol"^(-1) . What are the enthalpy of atomisation of NH_(3(g)) and the average bond enthalpy of N-H bond respectively ( in kJ "mol"^(-1) )?

Standard molar enthalpy of formation, Delta_(f) H^(Θ) is just a special case of enthalpy of reaction, Delta_(r) H^(Θ) . Is the Delta_(r) H^(Θ) same as standard molar enthalpy of formation ? Given reason for your answer. CaO (s) + CO_(2) (g) rarr CaCO_(3) (s) , Delta_(f) H^(Θ) = - 178.3 kJ mol^(-1)

The standard heat of formation (Delta_(f)H_(298)^(0)) of ethane (in kJ/mol), if the heat of combustion of ethane, hydrogen and graphite are -1560, -393.5 and -286kJ/mol , respectively is _______.

The standared enthalpies of formation at 298K for C C1(g), H_(2)O(g), CO_(2)(g) and HC1(g) are -106.7, -241.8, -393.7 , and -92.5kJ mol^(-1) , respectively. Calculate DeltaH^(Theta)underset(298K) for the reaction C C1_(4)(g) +2H_(2)O(g) rarr CO_(2)(g) +4HCI_(g)

The standard enthalpies of formation at 298K for C Cl(g), H_(2)O(g), CO_(2)(g) and HCl(g) are -106.7, -241.8, -393.7 , and -92.5kJ mol^(-1) , respectively. Calculate DeltaH^(Theta)underset(298K) for the reaction C Cl_(4)(g) +2H_(2)O(g) rarr CO_(2)(g) +4HCI(g)

The enthalpy of reaction for the reaction 2H_(2) (g) + O_(2) (g) rarr 2H_(2) O (l) " is " Delta_(r) H^(Θ) = - 572 kJ mol^(-1) What will be standard enthalpy of formation of H_(2) O (l) ?