From given following equations and $\Delta \mathrm{H}^{\circ}$ values, determine the enthalpy of reaction at…

From given following equations and $\Delta \mathrm{H}^{\circ}$ values, determine the enthalpy of reaction at $298 \mathrm{~K}$ for the reaction :
$\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})+6 \mathrm{~F}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{CF}_{4}(\mathrm{~g})+4 \mathrm{HF}(\mathrm{g})$
$\mathrm{H}_{2}(\mathrm{~g})+\mathrm{F}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{HF}(\mathrm{g}) ; \Delta \mathrm{H}_{1}^{\circ}=-537 \mathrm{~kJ}$
$\mathrm{C}(\mathrm{s})+2 \mathrm{~F}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CF}_{4}(\mathrm{~g}) ; \Delta \mathrm{H}_{2}^{\circ}=-680 \mathrm{~kJ}$
$2 \mathrm{C}(\mathrm{s})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g}) ; \Delta \mathrm{H}_{3}^{\circ}=52 \mathrm{~kJ}$
  1. $-1165$
  2. $-2486$
  3. $+1165$
  4. $+2486$

Solution

$\Delta \mathrm{H}^{\circ}=2 \times \Delta \mathrm{H}_{1}^{\circ}+2 \times \Delta \mathrm{H}_{2}^{\circ}-\Delta \mathrm{H}_{3}^{\circ}=-2486 \mathrm{~kJ}$

Asked in: JEE-TOPICTESTS-CHEMISTRY

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