JEE CHEMISTRY MCQ: Equilibrium

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Application +4 | -1

0.15

mole of CO taken in a

2.5 \mathrm{~L}

flask is maintained at

750 \mathrm{~K}

along with a catalyst so that the following reaction can take place.

\mathrm{CO}(g)+2 \mathrm{H}_2(g) \rightleftharpoons \mathrm{CH}_3 \mathrm{OH}(g)

Hydrogen is introduced until the total pressure of the system is

8.5 \mathrm{~atm}

at equilibrium and 0.08 mole of

\mathrm{CH}_3 \mathrm{OH}

are formed. The value of

K_c

is .....

\mathrm{mol}^{-2} \mathrm{~L}^{-2}

(Assigning ideal behaviour).

View answer and explanation

Correct option: A

187.85

Option A (187.85) is correct because it's the calculated value of Kc based on the equilibrium concentrations of the reactants and products.

More Questions from Equilibrium

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\mathrm{K}_1

\mathrm{K}_2

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

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

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

\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}

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

\mathrm{pH}

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

\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

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

\text{O}_2