The H - H bond energy is 430 kJ mol -1 and Cl-Cl bond energy is 240 kJ mol -1, Δ H for HCl is -90 kJ . The H - Cl bond energy is about :

Question

The H - H bond energy is 430 kJ mol -1 and Cl-Cl bond energy is 240 kJ mol -1, Δ H for HCl is -90 kJ . The H - Cl bond energy is about : (A) 180 kJ mol -1 (B) 360 kJ mol -1 (C) 213 kJ mol -1 (D) 425 kJ mol -1

Tardigrade Admin · Accepted Answer

The formation of one mole of HCl can be represented as, (1/2)( H - H )+(1/2)( Cl - Cl ) longrightarrow H - Cl ; Δ H=-90 kJ Hence, for the reaction, Heat evolved = heat evolved in bond formation - heat required for bond breaking ∴ 90 kJ =[ H - Cl bond energy] -((1/2) × 430+(1/2) × 24) ∴ ( H - Cl text bond energy )=90+(215+120) =425 kJ mol -1 .

Q. The $H - H$ bond energy is $430 k J m o l^{- 1}$ and $Cl - Cl$ bond energy is $240 k J m o l^{- 1}, Δ H$ for $H Cl$ is $- 90 k J .$ The $H - Cl$ bond energy is about :

$180 k J m o l^{- 1}$

$360 k J m o l^{- 1}$

$213 k J m o l^{- 1}$

$425 k J m o l^{- 1}$

Q. The H−H bond energy is 430kJmol−1 and Cl−Cl bond energy is 240kJmol−1,ΔH for HCl is −90kJ. The H−Cl bond energy is about :

180kJmol−1

360kJmol−1

213kJmol−1

425kJmol−1

Q. The $H - H$ bond energy is $430 k J m o l^{- 1}$ and $Cl - Cl$ bond energy is $240 k J m o l^{- 1}, Δ H$ for $H Cl$ is $- 90 k J .$ The $H - Cl$ bond energy is about :

$180 k J m o l^{- 1}$

$360 k J m o l^{- 1}$

$213 k J m o l^{- 1}$

$425 k J m o l^{- 1}$