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JEE Advanced levelSingle correct optionDifficulty 3 of 3ph077

Use the average bond enthalpies Cl-Cl $= 242$ , F-F $= 158$ and Cl-F $= 255 kJ mo l^{- 1}$ . The heat evolved when $3.55 g$ of $Cl X_{2}$ ( $M = 71 g mo l^{- 1}$ ) reacts completely with excess $F X_{2}$ according to $Cl X_{2} + F X_{2} 2 ClF$ is

A $0.55 kJ$
B $5.50 kJ$
C $11.00 kJ$
D $2.75 kJ$

Answer: B

Δ H = (242 + 158) - 2 (255) = - 110 kJ

per mole of

Cl X_{2}

(energy released is 110 kJ). Moles of

Cl X_{2} = 3.55/71 = 0.05

. Heat evolved

= 0.05 \times 110 = 5.50 kJ

.

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