Class 11Chemistry6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)
DifficultIn a $10 \ L$ vessel,$1 \ mol$ each of $PCl_5$ and $PCl_3$ are present. If the vessel is heated,some $PCl_5$ dissociates. What are the concentrations of $PCl_5$,$PCl_3$,and $Cl_2$ at equilibrium,respectively?
- A$0.1(1 - x), 0.1(1 + x)$ and $0.1x$
- B$0.2(1 - x), 0.2(1 + x)$ and $0.2x$
- C$0.3(1 - x), 0.3(1 + x)$ and $0.1x$
- DNone of the above
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Similar Questions
Match the items in List-$X$ with List-$Y$ and select the correct option.
List-$X$ List-$Y$ $(A)$ $A_{(g)} \rightleftharpoons B_{(g)} + \text{Heat}$ $(i)$ Equilibrium constant $(B)$ $r_b/r_f$ $(ii)$ Favored at low temperature $(C)$ $r_f/r_b$ $(iii)$ [Equilibrium constant]$^{-1}$ $(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)}$ $(iv)$ $A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$ $(E)$ Effect of pressure $(V)$ $\Delta n < 0$
| List-$X$ | List-$Y$ |
| $(A)$ $A_{(g)} \rightleftharpoons B_{(g)} + \text{Heat}$ | $(i)$ Equilibrium constant |
| $(B)$ $r_b/r_f$ | $(ii)$ Favored at low temperature |
| $(C)$ $r_f/r_b$ | $(iii)$ [Equilibrium constant]$^{-1}$ |
| $(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)}$ | $(iv)$ $A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$ |
| $(E)$ Effect of pressure | $(V)$ $\Delta n < 0$ |
Medium
View Solution$3.00 \ mol$ of $PCl_5$ kept in $1 \ L$ closed reaction vessel was allowed to attain equilibrium at $380 \ K$. If $1.59 \ mol$ of reactant was converted into the product at equilibrium,then $K_c$ is:
Medium
View SolutionIn a $1 \, L$ container,the reaction of $2 \, mol$ $N_2$ and $5 \, mol$ $H_2$ occurs. If the equilibrium concentration of $NH_3$ is half the equilibrium concentration of $N_2$,what is the equilibrium constant $(K_c)$?
Difficult
View SolutionConsider the following reaction equilibrium:
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
Initially,$1 \ mol$ of $N_2$ and $3 \ mol$ of $H_2$ are taken in a $2 \ L$ flask. At equilibrium,if the number of moles of $N_2$ is $0.6$,what is the total number of moles of all gases present in the flask?
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
Initially,$1 \ mol$ of $N_2$ and $3 \ mol$ of $H_2$ are taken in a $2 \ L$ flask. At equilibrium,if the number of moles of $N_2$ is $0.6$,what is the total number of moles of all gases present in the flask?
At $1000 \ K$ in a $0.654 \ L$ vessel,$CaCO_{3(s)}$ is taken. For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,the equilibrium constant $K_p$ is $3.9 \times 10^{-2} \ bar$. Find the weight of $CaO$ produced at equilibrium. $(Ca=40, C=12, O=16)$
Medium
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