The $C l_{2} O$ decompose spontaneously into elements because (Bond energies $C l - O = 50 K c a l / m o l, (O = O) = 119.2 K . C a l / m o l a n d C l - C l = 58 K . C a l / m o l$ )

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Heat is liberated in decomposition

Decomposition reaction is endothermic

Unstable reactant convert into stable products

Entropy increases in the decomposition

answer is B, C, D.

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Detailed Solution

$C l_{2} O \to C l_{2} + \frac{1}{2} O_{2}$

$Δ H = 2 D (C l - O) - D (C l - C l) - \frac{1}{2} D (O_{2})$

$= 2 (50 K . C a l / m o l) - (58 K . C a l / m o l) - \frac{1}{2} (119.2 K . C a l / m o l) = 2 (50 K . c a l / m o l) - (58 K . c a l / m o l) - \frac{1}{2} (119.2 K . c a l / m o l) = - 18 K . C a l$

The decomposition reaction with tend to be spontaneous if the energy change is negative. The enthalpy portion of the free energy change is negative, and the entropy change is positive, because more number gas molecules is produced upond decomposition. Since $Δ G = Δ H - T Δ S,$ the positive value of $Δ S$ and the negative value of $Δ H$ ensure that $Δ G$ will be negative.