First and second ionization enthalpies of lithium are $520 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $7297 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. Energy required to convert 3.5 mg lithium (g) into $\mathrm{Li}^{2+}(\mathrm{g})\left[\mathrm{Li}(\mathrm{g}) \rightarrow \mathrm{Li}^{2+}(\mathrm{g})\right]$ is $\_\_\_\_$ $\mathrm{kJ} \mathrm{mol}^{-1}$. (nearest integer)

[Molar mass of $\mathrm{Li}=7 \mathrm{~g} \mathrm{~mol}^{-1}$ ]

$$ \text { Consider the following sequence of reactions. } $$

The percentage of nitrogen in the yellow product $(\mathrm{X})$ formed is $\_\_\_\_$ $\%$.

(Nearest Integer)

(Given Molar mass in $\mathrm{g} \mathrm{mol}^{-1} \mathrm{H}: 1, \mathrm{C}: 12, \mathrm{~N}: 14$ )

4.7 g of phenol is heated with Zn to give product X . If this reaction goes to $60 \%$ completion then the number of moles of compound X formed will be

$\_\_\_\_$ $\times 10^{-2}$.(Nearest Integer)

(Given molar mass in $\mathrm{g} \mathrm{mol}^{-1}: \mathrm{H}: 1, \mathrm{C}: 12, \mathrm{O}: 16$ )

Sucrose hydrolyses in acidic medium into glucose and fructose by first order rate law with $t_{1 / 2}=3$ hour. The percentage of sucrose remaining after 6 hours is

$\_\_\_\_$ . (Nearest integer)

(Given $: \log 2=0.3010$ and $\log 3=0.4771$ )