Enthalpy change for the reaction, 4 H ( g ) arrow 2 H 2( g ) is -869.6 kJ The dissociation energy of H - H bond is

Question

Enthalpy change for the reaction, 4 H ( g ) arrow 2 H 2( g ) is -869.6 kJ The dissociation energy of H - H bond is (A) - 434.8 kJ (B) - 869.6 kJ (C) + 434.8 kJ (D) + 217.4 kJ

Tardigrade Admin · Accepted Answer

Given 4H(g) → 2H2(g) ; Δ H = - -869.6 kJ or 2H2 (g) → 4H(g) ; Δ H = 869.6 kJ H2 (g) → 2H(g) ; Δ H = (869.6/2) = 434.8 kJ

Q. Enthalpy change for the reaction,
$4 H_{(g)} \to 2 H_{2 (g)}$ is $- 869.6 k J$
The dissociation energy of $H - H$ bond is

- 434.8 kJ

- 869.6 kJ

+ 434.8 kJ

+ 217.4 kJ

Given
$4 H (g) \to 2 H_{2} (g); Δ H = - - 869.6 k J$
or $2 H_{2} (g) \to 4 H (g); Δ H = 869.6 k J$
$H_{2} (g) \to 2 H (g); Δ H = \frac{869.6}{2} = 434.8 k J$

Q. Enthalpy change for the reaction, 4H(g)​→2H2(g)​ is −869.6kJ The dissociation energy of H−H bond is