JEE CHEMISTRY MCQ: THERMODYNAMICS

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\begin{aligned} & \text {If } \mathrm{H}_2+1 / 2 \mathrm{O}_2 \longrightarrow \mathrm{H}_2 \mathrm{O}, \Delta \mathrm{H}=-68 \mathrm{~kcal} \\ & \mathrm{K}+\mathrm{H}_2 \mathrm{O}+\text {water} \longrightarrow \mathrm{KOH}(\mathrm{aq})+1 / 2 \mathrm{H}_2, \Delta \mathrm{H}=-48 \mathrm{~kcal} \\ & \mathrm{KOH}+\text {water} \longrightarrow \mathrm{KOH}(\mathrm{aq}), \Delta \mathrm{H}=-14 \mathrm{~kcal} \end{aligned}

Find the heat of formation of

\mathrm{KOH}

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Correct option: A

-102 k cal

Option A (-102 k cal) is correct because it is calculated by manipulating the given equations to arrive at the formation of KOH.

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\ \mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})-\mathrm{CO}(\mathrm{g}), \Delta \mathrm{H}_1=\mathrm{a}

\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})-\mathrm{CO}_2(\mathrm{~g}), \Delta \mathrm{H}_2=\mathrm{b}

\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})-2 \mathrm{CO}(\mathrm{g}) ; \Delta \mathrm{H}_3=\mathrm{c}

0.18 \mathrm{~g}

4 \mathrm{~K}.

\left(\Delta_{\mathrm{C}} \text{H}^{\circ}=-2.8\times 10^6 \mathrm{~J} / \mathrm{mol} \text{ glucose}\right)

{CsI}

{CsCl}

{CsCl}

{Cs} I

\begin{array}{cccccccccccccccccccc} {}&{\Delta H(KJ/mol)} \\ {1/2A \to B}&{ + 150} \\ {3B \to 2C + D}&{ - 125} \\ {E + A \to 2D}&{ + 350} \end{array}

{B}+{D} \rightarrow {E}+2 {C}, \Delta {H}

\Delta H

\Delta u

\mathrm{C}{\mathrm{H}_4}\left( \mathrm{g} \right) + 2{\mathrm{O}_2}\left( \mathrm{g} \right) \to \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) + {\mathrm{H}_2}\mathrm{O}\left( l \right);\Delta H = - 890.3\mathrm{kJ}