The exothermic formation of ${\rm{Cl}}{{\rm{F}}_3}$ is represented by the equation ${\rm{C}}{{\rm{l}}_2}\left( {\rm{g}} \right) + 3{{\rm{F}}_2}\left( {\rm{g}} \right)\leftrightharpoons2{\rm{Cl}}{{\rm{F}}_3}\left( {\rm{g}} \right);$ $\Delta H = - 329\,{\rm{kJ}}$ Which of the following will increase the quantity of ${\rm{Cl}}{{\rm{F}}_3}$ in an equilibrium mixture of ${\rm{C}}{{\rm{l}}_2},{{\rm{F}}_2}{\rm{and Cl}}{{\rm{F}}_3}$?

Increasing the volume of the container

Removing ${\rm{C}}{{\rm{l}}_2}$

JEE CHEMISTRY MCQ: Equilibrium

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Application +4 | -1

The exothermic formation of

\mathrm{Cl}{\mathrm{F}_3}

is represented by the equation

\mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) + 3{\mathrm{F}_2}\left( \mathrm{g} \right)\leftrightharpoons2\mathrm{Cl}{\mathrm{F}_3}\left( \mathrm{g} \right);

\Delta H = - 329\,\mathrm{kJ}

Which of the following will increase the quantity of

\mathrm{Cl}{\mathrm{F}_3}

in an equilibrium mixture of

\mathrm{C}{\mathrm{l}_2},{\mathrm{F}_2}\mathrm{and Cl}{\mathrm{F}_3}

View answer and explanation

Correct option: A

Adding

{\mathrm{F}_2}

Option A (Adding

{\mathrm{F}_2}

) is correct because, according to Le Chatelier's principle, adding a reactant to an exothermic reaction at equilibrium will shift the equilibrium towards the products.

More Questions from Equilibrium

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The indicator used in titrating oxalic acid with caustic soda solution is:

\mathrm{K}_1

and

\mathrm{K}_2

are equilibrium constant for reactions (i) and (ii)

\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})\quad\ldots

(i)

\mathrm{NO}(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{~N}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})\quad\ldots

(ii)

Then,

K{a_1},\,\,\,K{a_2}\,\,\,\mathrm{and}\,\,\,K{a_3}

are the respective ionisation constants for the following reactions

\begin{array}{l} {H_2}S\leftrightharpoons{H^ + } + H{S^ - }\\ H{S^ - }\leftrightharpoons{H^ + } + {S^{2 - }}\\ {H_2}S\leftrightharpoons2{H^ + } + {S^{2 - }} \end{array}

The correct relationship between

K{a_1},\,\,K{a_2}\,,K{a_3}

is The

\mathrm{pH}

0.1 \mathrm{~M}-\mathrm{N}_2 \mathrm{H}_4

solution is (For

\mathrm{N}_2 \mathrm{H}_4,

K_{{b}_1}=3.6 \times 10^{-6}, K_{{b}_2}=6.4 \times 10^{-12}, \log 2=0.3

\log 3=0.48

) Reaction

{\text{Ba}}{{\text{O}}_2}(s) \rightleftharpoons {\text{BaO}}(s) + {{\text{O}}_2}(g);\Delta H = - {\text{ve}}.

In equilibrium condition pressure of

\text{O}_2

depends on: A : At equilibrium concentration of the reactant and product does not change with time for a chemical reaction.
R: The rate of reaction is zero at equilibrium.