Class 11Chemistry6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)
Difficult$K_{c}$ for the following reaction is $99.0$: $A_{2(g)} \rightleftharpoons B_{2(g)}$. In a $1 \ L$ flask,$2 \ moles$ of $A_{2}$ were heated to $T(K)$ and equilibrium was reached. The concentrations at equilibrium of $A_{2}$ and $B_{2}$ are $C_{1}(A_{2})$ and $C_{2}(B_{2})$ respectively. Now,$1 \ mole$ of $A_{2}$ was added to the flask and heated to $T(K)$ to establish equilibrium again. The concentrations of $A_{2}$ and $B_{2}$ are $C_{3}(A_{2})$ and $C_{4}(B_{2})$ respectively. What is the value of $C_{3}(A_{2})$ in $mol \ L^{-1}$?
- A$0.01$
- B$0.03$
- C$0.02$
- D$2.97$
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The following lists contain reactions and their corresponding equilibrium constants at different temperatures:
List-$I$ (Reaction) List-$II$ $(K_p)$ $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $298 \ K$ $4.0 \times 10^{24}$ $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $700 \ K$ $3.0 \times 10^{4}$ $N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ at $298 \ K$ $0.98$ $N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ at $500 \ K$ $1700$
If $\Delta H_1^0$ and $\Delta H_2^0$ are the standard enthalpies for the reactions $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ and $N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ respectively, then:
| List-$I$ (Reaction) | List-$II$ $(K_p)$ |
|---|---|
| $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $298 \ K$ | $4.0 \times 10^{24}$ |
| $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $700 \ K$ | $3.0 \times 10^{4}$ |
| $N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ at $298 \ K$ | $0.98$ |
| $N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ at $500 \ K$ | $1700$ |
If $\Delta H_1^0$ and $\Delta H_2^0$ are the standard enthalpies for the reactions $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ and $N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ respectively, then:
The equilibrium constants $K_{p1}$ and $K_{p2}$ for the reactions $X \rightleftharpoons 2Y$ and $Z \rightleftharpoons P + Q$ respectively are in the ratio of $1 : 9$. If the degree of dissociation of $X$ and $Z$ be equal,then the ratio of total pressures at these equilibria is:
Match List-$I$ (Equations) with List-$II$ (Type of processes) and select the correct option.
List-$I$ (Equations) List-$II$ (Type of processes) $A. K_p > Q$ $(i)$ Non-spontaneous $B. \Delta G^\circ < RT \ln Q$ $(ii)$ Equilibrium $C. K_p = Q$ $(iii)$ Spontaneous and endothermic $D. T > \frac{\Delta H}{\Delta S}$ $(iv)$ Spontaneous
| List-$I$ (Equations) | List-$II$ (Type of processes) |
| $A. K_p > Q$ | $(i)$ Non-spontaneous |
| $B. \Delta G^\circ < RT \ln Q$ | $(ii)$ Equilibrium |
| $C. K_p = Q$ | $(iii)$ Spontaneous and endothermic |
| $D. T > \frac{\Delta H}{\Delta S}$ | $(iv)$ Spontaneous |
MediumAIPMT 2010
View SolutionFor the reaction $N_2 + O_2 \rightleftharpoons 2NO$ at $300 \, ^\circ C$,the value of $K_c$ is $9 \times 10^{-4}$. If equivalent amounts of $N_2$ and $O_2$ are used,what is the concentration of $NO$ at equilibrium (in terms of $a$) (in $, a$)?
Difficult
View SolutionWhich of the following equations is incorrect?
Medium
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