- A$1\%$ solution of glucose in water
- ✓$1\%$ solution of sodium chloride in water
- C$1\%$ solution of zinc sulphate in water
- D$1\%$ solution of urea in water
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Vapours $(B)+$ $\xrightarrow{{{K_2}{S_2}{O_8}}}\,(C)\, + \,(D)$
$(D)\,\xrightarrow{{(B)}}$ Brown $(E)$
Hybridisation of central atom in $(E)$ is


$[A]$ With increase in temperature, the value of $K$ for exothermic reaction decreases because entropy change of the system is positive
$[B]$ With increase in temperature, the value of $K$ for endothermic reaction increases because unfavourable change in entropy of the surroundings decreases
$[C]$ With increase in temperature, the value of $K$ for endothermic reaction increases because the entropy change of the system is negative
$[D]$ With increase in temperature, the value of $K$ for exothermic reaction decreases because favourable change in entropy of the surrounding decreases