JEE CHEMISTRY MCQ: THERMODYNAMICS

1 Hard

1 of 1

Analyzing +4 | -1

A solution of

500 \mathrm{~ml}

2 \mathrm{~M}-{KOH}

is added to

500 \mathrm{~ml}

2 \mathrm{~M}-{HCl}

and the mixture is well shaken. The rise in temperature

T_1

is noted. The experiment is again performed using

250 \mathrm{~ml}

{KOH}

solution and

500 \mathrm{~ml}

{HCl}

solution and rise in temperature

T_2

is again noted. Which of the following is correct?

View answer and explanation

Correct option: D

T_1

is 1.5 times as larger as

T_2

Option D (T1 is 1.5 times as larger as T2) is correct because the heat released in the first experiment is 1.5 times that of the second experiment.

More Questions from THERMODYNAMICS

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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}