The difference between enthalpy change and internal energy change for the combustion of one mole of ethyl alcohol is?

An athlete is given $100 \mathrm{g}$ of glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$ for energy. This is equivalent to $1800 \mathrm{kJ}$ of energy. The $50\%$ of this energy gained is utilized by the athlete for sports activities at the event. In order to avoid storage of energy, the weight of extra water he would need to perspire is $\mathrm{\_\_\_\_\_g}$ (Nearest integer) Assume that there is no other way of consuming stored energy.

Given : The enthalpy of evaporation of water is $45 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Molar mass of $\mathrm{C},\mathrm{H}\&\mathrm{O}$ are $12.1$ and $16 \mathrm{g} {\mathrm{mol}}^{-1}$.

The change in enthalpy $\left[\Delta \mathrm{H}\right]$ in ${\mathrm{kJmol}}^{-1}$ for the reaction is $\mathrm{Mg}+2 \mathrm{F}\to {\mathrm{MgF}}_2$

Given: $\mathrm{EA}$ of $\mathrm{F}=328 \mathrm{kJ} {\mathrm{mol}}^{-1},{\mathrm{IE}}_1$ of $\mathrm{Mg}=737 \mathrm{kJ} {\mathrm{mol}}^{-1},{\mathrm{IE}}_2$ of $\mathrm{Mg}=1451 \mathrm{kJ} {\mathrm{mol}}^{-1}$

The Born-Haber cycle for $\mathrm{KCl}$ is evaluated with the following data:
${\mathrm{\Delta }}_f{\mathrm{H}}^{\mathrm{\Theta }}\text{ for }\mathrm{KCl}=-436.7{\mathrm{kJmol}}^{-1};{\mathrm{\Delta }}_{\mathrm{sub}}{\mathrm{H}}^{\mathrm{\Theta }}\text{ for }\mathrm{K}=89.2{\mathrm{kJmol}}^{-1};$

${\mathrm{\Delta }}_{\text{ionization }}{\mathrm{H}}^{\mathrm{\Theta }}\text{ for }\mathrm{K}=419.0\mathrm{kJ}{\text{ mol }}^{-1};{\mathrm{\Delta }}_{\text{electron gain }}{\mathrm{H}}^{\mathrm{\Theta }}\text{ for }{\mathrm{Cl}}_{\left(\mathrm{g}\right)}=-348.6{\mathrm{kJmol}}^{-1}$

${\mathrm{\Delta }}_{\text{bond }}{\mathrm{H}}^{\mathrm{\Theta }}\text{ for }{\mathrm{Cl}}_2=243.0{\mathrm{kJmol}}^{-1}$
The magnitude of lattice enthalpy of $\mathrm{KCl}$ in ${\mathrm{kJmol}}^{-1}$ is (Nearest integer)

For one mole of NaCl(s) the lattice enthalpy is

${\mathrm{Na}}_{\left(\mathrm{s}\right)}+\frac{1}{2}{\mathrm{Cl}}_2\left(\mathrm{g}\right)\stackrel{+108.4 \mathrm{kJ}/\mathrm{mol}}{⟶}{\mathrm{Na}}_{\left(\mathrm{s}\right)}+\frac{1}{2}{\mathrm{Cl}}_2\left(\mathrm{g}\right)\stackrel{+495.6 \mathrm{kJ}/\mathrm{mol}}{⟶}{\mathrm{Na}}_{\left(\mathrm{g}\right)}^{+}+\frac{1}{2}{\mathrm{Cl}}_2\left(\mathrm{g}\right)\stackrel{121 \mathrm{kJ}/\mathrm{mol}}{⟶}$

${\mathrm{Na}}_{\left(\mathrm{g}\right)}^{+}+\mathrm{Cl}\left(\mathrm{g}\right)\stackrel{-348.6 \mathrm{kJ}/\mathrm{mol}}{⟶}{\mathrm{Na}}_{\left(\mathrm{g}\right)}^{+}+{\mathrm{Cl}}_{\left(\mathrm{g}\right)}^{-}\stackrel{{\mathrm{\Delta H}}^0 \mathrm{altice} }{⟶}\mathrm{Nacl}$ (solid) $\underset{-411.2 \mathrm{kJ}/\mathrm{mol}}{\leftarrow }{\mathrm{Na}}_{\left(\mathrm{s}\right)}+\frac{1}{2}{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

The standard heat of formation $\left({∆}_{\mathrm{f}}{\mathrm{H}}_{298}^0\right)$ of ethane is $-\frac{\mathrm{x}}{10}\mathrm{kJ}/\mathrm{mol}$, if the heat of combustion of ethane, hydrogen and graphite are $-1560,-393.5$ and $-\mathrm{286 }\mathrm{k}\mathrm{J}/\mathrm{m}\mathrm{o}\mathrm{l}$, respectively. The value of $\mathrm{x}$ to the nearest integer is_____

Tin is obtained from cassiterite by reduction with coke. Use the data given below to determine the minimum temperature (in $\mathrm{K}$) at which the reduction of cassiterite by coke would take place.

$298 \mathrm{K}: {\mathrm{\Delta }}_{\mathrm{f}}{\mathrm{H}}^0\left({\mathrm{SnO}}_2\left(\mathrm{s}\right)\right)=-581.0 \mathrm{kJ} {\mathrm{mol}}^{-1}, {\mathrm{\Delta }}_{\mathrm{f}}{\mathrm{H}}^0\left({\mathrm{CO}}_2\left(\mathrm{g}\right)\right)=-394.0 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{S}}^0\left({SnO}_2\left(\mathrm{s}\right)\right)=56.0 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}, {\mathrm{S}}^0\left(\mathrm{Sn}\right(\mathrm{s}\left)\right)=52.0 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$

${\mathrm{S}}^0\left(\mathrm{C}\right(\mathrm{s}\left)\right)=6.0 {\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}, {\mathrm{S}}^0\left({\mathrm{CO}}_2\left(\mathrm{g}\right)\right)=210.0 {\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}$

Assume that the enthalpies and the entropies are temperature independent.