One mole of ethanol ( $l$ ) was completely burnt in oxygen to form $\mathrm{CO}_2(\mathrm{~g})$ and $\mathrm{H}_2 \mathrm{O}(l)$. What is the $\Delta_r H^{\circ}$ (in $\mathrm{kJ} \mathrm{mol}^{-1}$ ) for this reaction?

(The standard enthalpy of formation $\left(\Delta_f H^{\circ}\right)$ of $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}(l), \mathrm{CO}_2(g)$ and $\mathrm{H}_2 \mathrm{O}(l)$ is respectively $-277,-393$ and $-286 \mathrm{~kJ} \mathrm{~mol}^{-1}$ )

If $\Delta_r H^{\ominus}$ and $\Delta_r S^{\ominus}$ are standard enthalpy change and standard entropy change respectively for a reaction, the incorrect option is

The $\mathrm{C}_p$ of $\mathrm{H}_2 \mathrm{O}(l)$ is $75.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$. What is the energy (in J ) required to raise 180 g of liquid water from $10^{\circ} \mathrm{C}$ to $15^{\circ} \mathrm{C}$ ? $\left(\mathrm{H}_2 \mathrm{O}=18 \mathrm{u}\right)$

Identify the incorrect statements from the following.

I. For adiabatic process, $\Delta U=w_{\text {ad }}$

II. Enthalpy is an intensive property

III. For the process, $\mathrm{H}_2 \mathrm{O}(l) \rightarrow \mathrm{H}_2 \mathrm{O}(s)$, the entropy increases

The correct answer is