Given that bond energies of H-H and Cl-Cl are 430 kJ mol-1 and 240 kJ mol-1 respectively and -fH for HCl is -90 kJ mol-1- Bond enthalpy of HCl is -

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Bond Order and Enthalpy

Given that bo...

Question

Given that bond energies of $H - H$ and $C l - C l$ are $430 k J m o l^{- 1}$ and $240 k J m o l^{- 1}$ respectively and $Δ_{f} H$ for $H C l$ is $- 90 k J m o l^{- 1}$ . Bond enthalpy of $H C l$ is :

245 k J m o l^{- 1}

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290 k J m o l^{- 1}

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380 k J m o l^{- 1}

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425 k J m o l^{- 1}

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Solution

The correct option is C $425 k J m o l^{- 1}$
Given :

Bond energies of $H - H$ and $C l - C l$ bonds which can be represented as follows :

$H_{2} (g) \to 2 H (g) Δ H_{(H)} = + 430 k J m o l^{- 1}$

$C l_{2} (g) \to 2 C l (g) Δ H_{(C l)} = + 240 k J m o l^{- 1}$

$H C l (g) \to H (g) + C l (g) Δ H_{(H c l)} = ?$

$\frac{1}{2} H_{2} + \frac{1}{2} C l_{2} \to H C l$

$Δ_{f} H_{H C l} = Δ H_{B E} R e a c t a n t + Δ H_{B E} P r o d u c t - B E$ of $H C l$

$\Rightarrow - 90 = \frac{1}{2} \times 430 + \frac{1}{2} \times 240 - B E$ of $H C l$

$\Rightarrow B E$ of $H C l = 215 + 120 + 90 = 305 + 120 = 425 k J m o l^{- 1}$

Where, $B E =$ Bond enthalpy

Hence, the correct option is D.

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Similar questions

Given that bond energies of
$H - H$ and $C l - C l$ are $430 k J m o l^{- 1}$ and $240 k J m o l^{- 1}$ respectively and $Δ_{f} H$ for $H C l$ is -90 kJ $m o l^{- 1} .$ The bond enthalpy of $H C l$ is:

Q. Given that bond energy of

H - H

and

C l - C l

are

430 k J

m o 1^{- 1}

and

240 k J

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respectively and heat of formation for

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- 90 k J

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is:

Q. Bond energies of H - H and CI - CI are

430 k J m o l^{- 1}

and

242 k J m o l^{- 1}

respectively.

Δ H_{f}

for HCl is

91 k J m o l^{- 1}

. What will be the bond energy of H - Cl bond (per mole value)?

Q. Given that, bond energies of

H - H

and

C l - C l

430 k J / m o l

and

240 k J / m o l

respectively.

Δ H_{f}

for

H C l

- 90 k J / m o l

. Bond enthalpy of

H C l

is:

Q. Calculate free energy change for the reaction at

27^{o} C

H_{2 (g)} + C l_{2 (g)} \to 2 H - C l_{(g)}

by using the bond energy and energy data.
Bond energies of

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and

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bonds are

435 k J m o l^{- 1}, 240 k J m o l^{- 1}

and

430 k J m o l^{- 1}

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respectively.

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Given that bond energies of H−H and Cl−Cl are 430 kJ mol−1 and 240 kJ mol−1 respectively and ΔfH for HCl is −90 kJ mol−1. Bond enthalpy of HCl is :

Given that bond energies of $H - H$ and $C l - C l$ are $430 k J m o l^{- 1}$ and $240 k J m o l^{- 1}$ respectively and $Δ_{f} H$ for $H C l$ is $- 90 k J m o l^{- 1}$ . Bond enthalpy of $H C l$ is :