JEE CHEMISTRY MCQ: THERMODYNAMICS

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Analyzing +4 | -1

When

1 \mathrm{~g}

equivalent of strong acid reacts with strong base, the heat released is

13.5 \mathrm{~kcal}.

When

1 \mathrm{~g}

equivalent

\mathrm{H}_2 \mathrm{A}

is completely neutralized against strong base,

13 \mathrm{~kcal}

is released. When

1 \mathrm{~g}

equivalent

\mathrm{B}(\mathrm{OH})_2

is completely neutralized against strong acid,

10 \mathrm{~kcal}

heat is released. What is the enthalpy change when 1 mole of

\mathrm{H}_2 \mathrm{A}

is completely neutralized by

\mathrm{B}(\mathrm{OH})_2?

View answer and explanation

Correct option: D

-19 \mathrm{~kcal}

The correct answer is D (-19 kcal) because the enthalpy change is calculated by considering the enthalpy of ionization for both the acid and the base and subtracting them from the total heat released during neutralization.

More Questions from THERMODYNAMICS

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Consider following reactions
I:

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

II:

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

III:

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

Select the correct statement When

0.18 \mathrm{~g}

of glucose was burnt in a bomb calorimeter, the temperature rose by

4 \mathrm{~K}.

The heat capacity of the calorimeter system is

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

Statement-1:

{CsI}

is less soluble in water compared to

{CsCl}

Satement-2: More amount of heat is liberated during the formation of

{CsCl}

than the formation

{Cs} I

from their elements Consider the following processes :

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

For

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

will be : The difference b/w

\Delta H

and

\Delta u

at constant volume is equal to The heat evolved in the combustion of methane is given by the following equations

\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}

How many grams of methane would be required to produce 44.15 kJ of heat of combustion?