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Standard XII

Chemistry

Enthalpy of Solution

The standard ...

Question

The standard enthalpy of formation (ΔfH°) 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

the dissociation energy of

H_{2}

and enthalpy of sublimation of carbon

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latent heat of vaporization of methane

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

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he dissociation energy of hydrogen molecule,

H_{2}

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Solution

The correct option is A the dissociation energy of $H_{2}$ and enthalpy of sublimation of carbon
Carbon is found in the solid-state. The state of the substance affects the enthalpy change.
Hence, the correct option is $A$

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Similar questions

The standard enthalpy of formation $(Δ_{f} H^{0})$ at 298K for methane, $C H_{4} (G)$ is 74.8kJmol $^{- 1}$ . The additional information required to determine the average energy for C-H bond formation would be

Q. The bond dissociation energies for

{C l}_{2}, I_{2}

and

I C l

are

242.3, 151

and

211.3

k J / m o l

respectively. The enthalpy of sublimation of iodine is

62.8 k J / m o l

. What is the standard enthalpy of formation of

I C l (g)

Q. Calculate the electron gain enthalpy of fluorine from the data given below.

Δ H_{f}

of KF is - 560.8 KJ/ mol, dissociation energy of

F_{2}

is 158.9 KJ / mol. Lattice energy of KF is 807.5 KJ/mol, ionization energy of potassium is 414.2 KJ/mol and enthalpy of sublimation of

K = 87.8 K J / m o l .

Q. Use the following data to calculate the lattice energy of caesium oxide.
Enthalpy of formation of caesium oxide

= - 233 kJ/mol

Enthalpy of sublimation of

C s = + 78 kJ/mol

First ionization energy of

C s = + 375 kJ/mol

Enthalpy of dissociation of

O_{2} (g) = 494 kJ/mol

First electron affinity of

O = - 141 kJ/mol

Second electron affinity of

O = + 845 kJ/mol

Q. Calculate the lattice enthalpy of

K C l

from the following data at standard states-
Enthalpy of sublimation of

K = 89 k J m o l^{- 1}

Enthalpy of dissociation of

C l_{2} = 244 k J m o l^{- 1}

Ionisation energy of

K = 425 k J m o l^{- 1}

Electron gain enthalpy of

C l = - 355 k J m o l^{- 1}

Enthalpy of formation of

K C l = - 438 k J m o l^{- 1}

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The standard enthalpy of formation (ΔfH°) at 298 K for methane, CH4(g), is –74.8 kJ mol–1. The additional information required to determine the average energy for C – H bond formation would be

The correct option is A the dissociation energy of H2 and enthalpy of sublimation of carbonCarbon is found in the solid-state. The state of the substance affects the enthalpy change.Hence, the correct option is A

The standard enthalpy of formation (ΔfH°) 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

The correct option is A the dissociation energy of $H_{2}$ and enthalpy of sublimation of carbon
Carbon is found in the solid-state. The state of the substance affects the enthalpy change.
Hence, the correct option is $A$