Given are the following thermochemical equations.

$\mathrm{Z}\mathrm{n}+\frac{1}{2}{\mathrm{O}}_2\to \mathrm{Z}\mathrm{n}\mathrm{O}+\mathrm{84,000}\mathrm{ }\mathrm{c}\mathrm{a}\mathrm{l}$

$\mathrm{H}\mathrm{g}+\frac{1}{2}{\mathrm{O}}_2\mathrm{ }\to \mathrm{H}\mathrm{g}\mathrm{O}+\mathrm{21,700}\mathrm{ }\mathrm{c}\mathrm{a}\mathrm{l}$

Accordingly, the heat of reaction for the following reaction, $\mathrm{Z}\mathrm{n}+\mathrm{H}\mathrm{g}\mathrm{O}\to \mathrm{H}\mathrm{g}+$heat is

Given

(A) $2\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to 2{\mathrm{CO}}_2\left(\mathrm{g}\right) {\mathrm{\Delta H}}_1^{\mathrm{o}}=-\mathrm{x} \mathrm{kJ} {\mathrm{mol}}^{-1}$

(B) $\mathrm{C}\left(\mathrm{graphite}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right) {\mathrm{\Delta H}}_2^{\mathrm{o}}=-\mathrm{y} \mathrm{kJ} {\mathrm{mol}}^{-1}$

The $∆{\mathrm{H}}^{\mathrm{o}}$ for the reaction $\mathrm{C}\left(\mathrm{graphite}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to \mathrm{CO}\left(\mathrm{g}\right)$ is

Consider the following data

Heat of combustion of ${\mathrm{H}}_2\left(\mathrm{g}\right)=–241.8 \mathrm{kJ} {\mathrm{mol}}^{–1}$

Heat of combustion of $\mathrm{C}\left(\mathrm{s}\right)=–393.5 \mathrm{kJ} {\mathrm{mol}}^{–1}$

Heat of combustion of  ${\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}\left(\mathrm{l}\right)$$=–1234.7 \mathrm{kJ} {\mathrm{mol}}^{–1}$

The heat of formation of ${\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}\left(\mathrm{l}\right)$ is $(–)$ _____ $\mathrm{kJ} {\mathrm{mol}}^{–1}$ (Nearest integer).

Solid fuel used in rocket is a mixture of ${\mathrm{Fe}}_2{\mathrm{O}}_3$and $\mathrm{Al}$ (in ratio $1 : 2$). The heat evolved $\left(\mathrm{kJ}\right)$ per gram of the mixture is _____ (Nearest integer)

Given ${\mathrm{\Delta H}}_{\mathrm{f}}^0\left({\mathrm{Al}}_2{\mathrm{O}}_3\right)=-1700 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{\Delta H}}_{\mathrm{f}}^0\left({\mathrm{Fe}}_2{\mathrm{O}}_3\right)=-840 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Molar mass of $\mathrm{Fe}, \mathrm{AI}$ and $\mathrm{O}$ are $56, 27$ and $16 \mathrm{g} {\mathrm{mol}}^{–1}$ respectively

At $25°\mathrm{C}$, the enthalpy of the following processes are given:

${\mathrm{H}}_2( \mathrm{g})+{\mathrm{O}}_2( \mathrm{g})\to 2\mathrm{OH}\left(\mathrm{g}\right)\Delta {\mathrm{H}}^{\mathrm{o}}=78 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{H}}_2( \mathrm{g})+1/2{\mathrm{O}}_2( \mathrm{g})\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\Delta {\mathrm{H}}^0=-242 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{H}}_2( \mathrm{g})\to 2\mathrm{H}\left(\mathrm{g}\right)\Delta {\mathrm{H}}^{\mathrm{o}}=436 \mathrm{kJ} {\mathrm{mol}}^{-1}$

$1/2{\mathrm{O}}_2( \mathrm{g})\to \mathrm{O}\left(\mathrm{g}\right)\Delta {\mathrm{H}}^0=249 \mathrm{kJ} {\mathrm{mol}}^{-1}$

What would be the value of X for the following reaction? (Nearest integer)

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\to \mathrm{H}\left(\mathrm{g}\right)+\mathrm{OH}\left(\mathrm{g}\right) ∆{\mathrm{H}}^{\mathrm{o}}=\mathrm{X} {\mathrm{kJmol}}^{-1}$

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)