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Spontaneity

Heat evolved ...

Question

Heat evolved in the reaction $H_{2} + C l_{2} \to 2 H C l$ is $182$ KJ. Bond energies of $H - H$ and $C l - C l$ are $430$ and $242$ KJ/mol respectively.

Thus $H - C l$ bond energy is :

245

m o l^{- 1}

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427

m o l^{- 1}

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336

m o l^{- 1}

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154

m o l^{- 1}

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Solution

The correct option is B $427$ KJ $m o l^{- 1}$
$Δ H_{f}$ $f o r H C l$ $i s - 182 K J / 2 = - 91 K J$

$\frac{1}{2} H_{2}$ $+$ $\frac{1}{2} C l_{2}$ $= H C L$

$Δ_{f} H$ = $Δ H_{B} E$ reactants - $Δ H_{B} E$ products

$- 91 = \frac{1}{2} \times 430 + \frac{1}{2} \times 242$ - $Δ H_{B} E$ products

$Δ H_{B} E$ products $= 91 + 215 + 121 = 427 K J m o l^{- 1}$

Hence, the correct option is B.

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Similar questions

Q. Heat evolved in the reaction

H_{2} + {C l}_{2} ⟶ 2 H C l

is 182 kJ. Bond energies pf H-H and Cl-Cl are 430 and 242 KJ/mol respectively. The H-Cl bond energy 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 kJ $m o l^{- 1} .$ The bond enthalpy of $H C l$ is:

Q. The

H - H

bond energy is 430 kJ mol

^{- 1}

and

C l - C l

bond energy is 240 kJ mol

^{- 1}

Δ H_{f}

H C l

- 90

kJ. The

H - C l

bond energy is

(420 + x)

kJ mol

^{- 1}

, where

x

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. Heat evolved in the reaction ,

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

182 k J

. Bond energies

H - H = 430 k J / m o l e

, and

C l - C l = 242 k J / m o l e

. The

H - C l

bond energy is

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Heat evolved in the reaction H2+Cl2→2HCl is 182 KJ. Bond energies of H−H and Cl−Cl are 430 and 242 KJ/mol respectively. Thus H−Cl bond energy is :

The correct option is B 427 KJ mol−1ΔHf for HCl is−182KJ/2=−91KJ12H2 + 12Cl2 =HCLΔfH = ΔHBE reactants - ΔHBE products−91=12×430+12×242 - ΔHBE productsΔHBE products =91+215+121=427KJmol−1Hence, the correct option is B.

Heat evolved in the reaction $H_{2} + C l_{2} \to 2 H C l$ is $182$ KJ. Bond energies of $H - H$ and $C l - C l$ are $430$ and $242$ KJ/mol respectively.

Thus $H - C l$ bond energy is :