For an endothermic reaction:

(A) $$\mathrm{q}_{\mathrm{p}}$$ is negative.

(B) $$\Delta_{\mathrm{r}} \mathrm{H}$$ is positive.

(C) $$\Delta_r \mathrm{H}$$ is negative.

(D) $$\mathrm{q}_{\mathrm{p}}$$ is positive.

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For the following reaction at $$300 \mathrm{~K}$$

$$\mathrm{A}_2(\mathrm{~g})+3 \mathrm{~B}_2(\mathrm{~g}) \rightarrow 2 \mathrm{AB}_3(\mathrm{~g})$$

the enthalpy change is $$+15 \mathrm{~kJ}$$, then the internal energy change is :

In which of the following processes entropy increases?

A. A liquid evaporates to vapour.

B. Temperature of a crystalline solid lowered from $$130 \mathrm{~K}$$ to $$0 \mathrm{~K}$$.

C. $$2 \mathrm{NaHCO}_{3(\mathrm{~s})} \rightarrow \mathrm{Na}_2 \mathrm{CO}_{3(\mathrm{~s})}+\mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$$

D. $$\mathrm{Cl}_{2(g)} \rightarrow 2 \mathrm{Cl}_{(g)}$$

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Match List I with List II.

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