Bond energies of few bonds are given below: Cl — Cl = 242.8 kJ mol-1, H — Cl = 431.8 kJ mol-1, O — H = 464 kJ mol-1, O = O = 442 kJ mol-1 Using the B.E., calculate Δ H for the following reaction, 2Cl2 + 2H2O → 4HCl + O2

Question

Bond energies of few bonds are given below: Cl — Cl = 242.8 kJ mol-1, H — Cl = 431.8 kJ mol-1, O — H = 464 kJ mol-1, O = O = 442 kJ mol-1 Using the B.E., calculate Δ H for the following reaction, 2Cl2 + 2H2O → 4HCl + O2 (A) 906 kJ mol-1 (B) 172.4 kJ mol-1 (C) 198.8 kJ mol-1 (D) 442 kJ mol-1

Tardigrade Admin · Accepted Answer

2Cl2 + 2H2O → 4HCl + O2 Δ H = B.E. of (2 × Cl — Cl) + (2 × 2 × O — H) - (4 × H — Cl) + (O = O) = 2 × 242.8 + 4 × 464 - 4 × 431.8 - 442 = 172.4 kj mol-1

Q. Bond energies of few bonds are given below :
$Cl — Cl = 242.8 k J m o l^{- 1}$ , $H — Cl = 431.8 k J m o l^{- 1,}$
$O — H = 464 k J m o l^{- 1}$ , $O = O = 442 k J m o l^{- 1}$
Using the $B . E .$ , calculate $Δ H$ for the following reaction, $2 C l_{2} + 2 H_{2} O \to 4 H Cl + O_{2}$

$906 k J m o l^{- 1}$

$172.4 k J m o l^{- 1}$

$198.8 k J m o l^{- 1}$

$442 k J m o l^{- 1}$

$2 C l_{2} + 2 H_{2} O \to 4 H Cl + O_{2}$
$Δ H = B . E .$ of $(2 \times Cl — Cl) + (2 \times 2 \times O — H)$
$- (4 \times H — Cl) + (O = O)$
$= 2 \times 242.8 + 4 \times 464 - 4 \times 431.8 - 442$
$= 172.4 kj m o l^{- 1}$

Q. Bond energies of few bonds are given below : Cl—Cl=242.8kJmol−1, H—Cl=431.8kJmol−1, O—H=464kJmol−1, O=O=442kJmol−1 Using the B.E., calculate ΔH for the following reaction, 2Cl2​+2H2​O→4HCl+O2​

906kJmol−1

172.4kJmol−1

198.8kJmol−1

442kJmol−1