Class 11Chemistry1 Equilibrium: Chemical EquilibriumMix Examples- 6-1.Equilibrium (Chemical Equilibrium)
MediumFor the reaction $CH_4(g) + 2O_2(g) \rightleftharpoons CO_2(g) + 2H_2O(l)$,the enthalpy change is $\Delta H_r = -170.8 \, kJ \, mol^{-1}$. Which of the following statements is $NOT$ true?
- AAt equilibrium,the concentrations of $CO_2(g)$ and $H_2O(l)$ are not equal.
- BThe equilibrium constant for the reaction is given by $K_p = \frac{P_{CO_2}}{P_{CH_4} \cdot P_{O_2}^2}$.
- CAdding $CH_4(g)$ or $O_2(g)$ at equilibrium shifts the reaction to the right.
- DThe reaction is exothermic.
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Similar Questions
For the reaction,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,if dinitrogen tetroxide is $50\%$ dissociated at $60^\circ C$,the standard free energy change at this temperature and $1 \ atm$ pressure is:
At $783 \, K$ in the reaction,$H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,the molar concentrations $(mol \, L^{-1})$ of $H_2, I_2$ and $HI$ at some instant of time are $0.1, 0.2$ and $0.4$,respectively. If the equilibrium constant is $46$ at the same temperature,then as the reaction proceeds:
MediumKVPY 2011
View SolutionIn a $2 \ L$ vessel,$1 \ mol$ of $H_2$ and $2 \ mol$ of $I_2$ are taken. If at equilibrium the moles of $H_2$ are $0.2$,then the moles of $I_2$ and $HI$ at equilibrium will be respectively:
Medium
View SolutionMatch the items in List-$X$ with List-$Y$ and select the correct option.
List-$X$ List-$Y$ $(A)$ Active mass $(i)$ $\Delta n = 0$ $(B)$ Equilibrium constant $(ii)$ Molar concentration $(C)$ $A + \text{Heat} \rightleftharpoons B$ $(iii)$ Van't Hoff equation $(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)}$ $(iv)$ Favoured by increase in temperature $(v)$ Chemical equilibrium
| List-$X$ | List-$Y$ |
| $(A)$ Active mass | $(i)$ $\Delta n = 0$ |
| $(B)$ Equilibrium constant | $(ii)$ Molar concentration |
| $(C)$ $A + \text{Heat} \rightleftharpoons B$ | $(iii)$ Van't Hoff equation |
| $(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)}$ | $(iv)$ Favoured by increase in temperature |
| $(v)$ Chemical equilibrium |
Medium
View SolutionThe equilibrium constant for the following reaction is $1.6 \times 10^{5}$ at $1024 \, K$:
$H_{2(g)} + Br_{2(g)} \longleftrightarrow 2HBr_{(g)}$
Find the equilibrium pressure of all gases if $10.0 \, bar$ of $HBr$ is introduced into a sealed container at $1024 \, K$.
$H_{2(g)} + Br_{2(g)} \longleftrightarrow 2HBr_{(g)}$
Find the equilibrium pressure of all gases if $10.0 \, bar$ of $HBr$ is introduced into a sealed container at $1024 \, K$.
Difficult
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