Data given for the following reaction is as follows :

${\mathrm{FeO}}_{\left(\mathrm{s}\right)}+{\mathrm{C}}_{\left(\mathrm{graphite}\right)}⟶{\mathrm{Fe}}_{\left(\mathrm{s}\right)}+{\mathrm{CO}}_{\left(\mathrm{g}\right)}$

Substance	${\Delta }_{\mathrm{f}}\mathrm{H}° \left({\mathrm{kJmol}}^{-1}\right)$	$\Delta \mathrm{S}° \left({\mathrm{Jmol}}^{-1} {\mathrm{K}}^{-1}\right)$
${\mathrm{FeO}}_{\left(\mathrm{s}\right)}$	$-266.3$	$57.49$
${\mathrm{C}}_{\left(\mathrm{graphite}\right)}$	$0$	$5.74$
${\mathrm{Fe}}_{\left(\mathrm{s}\right)}$	$0$	$27.28$
${\mathrm{CO}}_{\left(\mathrm{g}\right)}$	$-110.5$	$197.6$

The minimum temperature in $\mathrm{K}$ at which the reaction becomes spontaneous is_____.(Nearest integer)

$200 \mathrm{mL}$ of $0.2 \mathrm{M} \mathrm{HCl}$ is mixed with $300 \mathrm{mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}.$ The molar heat of neutralization of this reaction is $-57.1 \mathrm{kJ}.$ The increase in temperature in ${}^{\circ }\mathrm{C}$ of the system on mixing is $\mathrm{x}\times {10}^{-2}.$ The value of $\mathrm{x}$ is (Nearest integer)

[Given: Specific heat of water $=4.18 \mathrm{J} {\mathrm{g}}^{-1} {\mathrm{K}}^{-1}$ 

Density of water$=1.00 \mathrm{g}{ \mathrm{cm}}^{-3}$]

(Assume no volume change on mixing)

The average $\mathrm{S}-\mathrm{F}$ bond energy in $\mathrm{kJ} {\mathrm{mol}}^{-1}$ of ${\mathrm{SF}}_6$ is _. (Rounded off to the nearest integer)

[Given : The values of standard enthalpy of formation of ${\mathrm{SF}}_6\left(\mathrm{g}\right), \mathrm{S}\left(\mathrm{g}\right)$ and $\mathrm{F}\left(\mathrm{g}\right)$ are $-1100, 275$ and $80 \mathrm{kJ} {\mathrm{mol}}^{-1}$ respectively.]

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)

[ Use $R=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$]