Δ H for the reaction, OF2 + H2O → O2 + 2HF (B.E. of O — F, O — H, H — F and O = O are 44, 111, 135 and 119 kcal mol-1 respectively)

Question

Δ H for the reaction, OF2 + H2O → O2 + 2HF (B.E. of O — F, O — H, H — F and O = O are 44, 111, 135 and 119 kcal mol-1 respectively) (A) - 222 kcal (B) - 88 kcal (C) - 111 kcal (D) - 79 kcal

Tardigrade Admin · Accepted Answer

Δ H = Sigma B.E.R - Sigma B.E.P = (2 × 44 + 2 × 111) - (119 + 2 × 135) = - 79 kcal

Q. $Δ H$ for the reaction, $O F_{2} + H_{2} O \to O_{2} + 2 H F$
$(B . E .$ of $O — F$ , $O — H$ , $H — F$ and $O = O$ are $44$ , $111$ , $135$ and $119 k c a l m o l^{- 1}$ respectively)

$- 222 k c a l$

$- 88 k c a l$

$- 111 k c a l$

$- 79 k c a l$

$Δ H = Σ B . E ._{R} - Σ B . E ._{P}$
$= (2 \times 44 + 2 \times 111) - (119 + 2 \times 135)$
$= - 79 k c a l$

Q. ΔH for the reaction, OF2​+H2​O→O2​+2HF (B.E. of O—F, O—H, H—F and O=O are 44, 111, 135 and 119kcalmol−1 respectively)

−222kcal

−88kcal

−111kcal

−79kcal