For the equilibrium, $ \mathrm{C}(\mathrm{s})+\mathrm{CO}_2(g) \rightleftharpoons 2 \mathrm{CO}(g) ; K_p=63 \mathrm{~atm} $ at $1000 \mathrm{~K}$ if at equilibrium $p_{\mathrm{CO}}=10 p_{\mathrm{CO}_2}$ then total pressure at equilibrium is

JEE CHEMISTRY MCQ: Equilibrium

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For the equilibrium,

\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(g) \rightleftharpoons 2 \mathrm{CO}(g) ; K_p=63 \mathrm{~atm}

1000 \mathrm{~K}

if at equilibrium

p_{\mathrm{CO}}=10 p_{\mathrm{CO}_2}

then total pressure at equilibrium is

View answer and explanation

Correct option: C

6.93 atm

Option C (6.93 atm) is correct because it is the sum of the partial pressures of CO and CO2 at equilibrium, calculated using the given Kp and the relationship between the partial pressures.

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.