What is bond dissociate energy of HCl- - Hf HCl - -93- B-E- H2 - 434- B-E- Cl2 - 242 in KJ- mol

The correct option is D 431 KJ/mol 12 H_2 + 12 Cl_2 → HCl #160; Δ H_f Δ H_f = B.E.H_2 ×12 + B.E.Cl_2 ×12 B.E. HCl ...

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Standard XII

Chemistry

Enthalpy

What is bond ...

Question

What is bond dissociate energy of HCl, $Δ H_{f} (H C l) = - 93, B . E . (H_{2}) = 434, B . E . (C l_{2}) = 242$ (in KJ/ mol)

532 KJ/mol

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431 KJ/mol

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332 KJ/mol

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232 KJ/mol

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Solution

The correct option is D 431 KJ/mol
$\frac{1}{2} H_{2} + \frac{1}{2} C l_{2} \to H C l$ $Δ H_{f}$
$Δ H_{f} = B . E . H_{2} \times \frac{1}{2} + B . E . C l_{2} \times \frac{1}{2} - B . E . H C l$

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Similar questions

Q. Find the enthalpy of formation of Hydrogen flouride on the basis of following data :
Bond energy of

H - H = 434 k J m o l^{- 1}

Bond energy of

F - F = 158 k J m o l^{- 1}

Bond energy of

H - F = 565 k J m o l^{- 1}

Q. Bond dissociation enthalpy of

H_{2}, C l_{2}

and

H C l

are 434, 242 and 431 kJ

m o l^{- 1}

respectively.

Enthalpy of formation of

H C l

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. Calculate the enthalpy change for the reaction,

H_{2} + F_{2} \to 2 H F

given that
Bond energy of H – H bond = 434 kJ/mol
Bond energy of F – F bond = 158 kJ/mol
Bond energy of H – F bond = 565 kJ/mol

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:

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What is bond dissociate energy of HCl, ΔHf(HCl)=−93,B.E.(H2)=434,B.E.(Cl2)=242 (in KJ/ mol)

The correct option is D 431 KJ/mol12H2+12Cl2→HCl ΔHfΔHf=B.E.H2×12+B.E.Cl2×12−B.E.HCl

What is bond dissociate energy of HCl, $Δ H_{f} (H C l) = - 93, B . E . (H_{2}) = 434, B . E . (C l_{2}) = 242$ (in KJ/ mol)

The correct option is D 431 KJ/mol
$\frac{1}{2} H_{2} + \frac{1}{2} C l_{2} \to H C l$ $Δ H_{f}$
$Δ H_{f} = B . E . H_{2} \times \frac{1}{2} + B . E . C l_{2} \times \frac{1}{2} - B . E . H C l$