What will be Δ H for the reaction, CH2Cl2 → C + 2H + 2Cl ? (B.E. of C — H and C — Cl bonds are 416 kJ mol-1 and 325 kJ mol-1 respectively)

Question

What will be Δ H for the reaction, CH2Cl2 → C + 2H + 2Cl ? (B.E. of C — H and C — Cl bonds are 416 kJ mol-1 and 325 kJ mol-1 respectively) (A) 832 kJ (B) 1482 kJ (C) 650 kJ (D) 1855 kJ

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/633800fb616d69fe962518206203005a-.jpeg" /> Δ H = Sigma B.E.R - Sigma B.E.P =2× B.E. (C — H) + 2 × B.E. (C — Cl) = 2 × 416 + 2 × 325 = 1482 kJ

Q. What will be $Δ H$ for the reaction,
$C H_{2} C l_{2} \to C + 2 H + 2 Cl ?$
$(B . E .$ of $C — H$ and $C — Cl$ bonds are $416 k J m o l^{- 1}$ and $325 k J m o l^{- 1}$ respectively)

$832 k J$

$1482 k J$

$650 k J$

$1855 k J$

$Δ H = Σ B . E ._{R} - Σ B . E ._{P}$
$= 2 \times B . E . (C — H) + 2 \times B . E . (C — Cl)$
$= 2 \times 416 + 2 \times 325 = 1482 k J$

Q. What will be ΔH for the reaction, CH2​Cl2​→C+2H+2Cl? (B.E. of C—H and C—Cl bonds are 416kJmol−1 and 325kJmol−1 respectively)

832kJ

1482kJ

650kJ

1855kJ