The equilibrium constants for $\mathrm{A}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{A}(\mathrm{g})$ at $400 \mathrm{~K}$ and $600 \mathrm{~K}$ are $1 \times 10^{-8}$ and $1 \times 10^{-2}$ respectively. The reaction is

May be exothermic or endothermic

JEE CHEMISTRY MCQ: Equilibrium

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Analyzing +4 | -1

The equilibrium constants for

\mathrm{A}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{A}(\mathrm{g})

400 \mathrm{~K}

and

600 \mathrm{~K}

are

1 \times 10^{-8}

and

1 \times 10^{-2}

respectively. The reaction is

View answer and explanation

Correct option: B

Endothermic

The correct answer is Endothermic because the equilibrium constant increases with increasing temperature, indicating that heat is absorbed, favoring product formation.

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.