Class 11Chemistry6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)
Medium$S_1$: In case of endothermic reactions,the equilibrium shifts in the forward direction on increasing temperature.
$S_2$: The value of $K_{eq}$ depends only on temperature and is independent of pressure.
$S_3$: For the reaction,$H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$,the equilibrium constant,$K_{eq}$ is dimensionless because the number of moles of gaseous products equals the number of moles of gaseous reactants.
$S_2$: The value of $K_{eq}$ depends only on temperature and is independent of pressure.
$S_3$: For the reaction,$H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$,the equilibrium constant,$K_{eq}$ is dimensionless because the number of moles of gaseous products equals the number of moles of gaseous reactants.
- A$T, F, F$
- B$F, T, F$
- C$T, T, F$
- D$F, F, T$
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For the reaction $C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)}$,if $25\%$ of $CO_2$ is converted to $CO$ at equilibrium and the total equilibrium pressure is $12 \ atm$,then the partial pressure of $CO_2$ at equilibrium will be............$atm$.
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View SolutionThe 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:
If the volume of the container for the reaction $2NO + O_2 \rightleftharpoons 2NO_2$ is reduced to half of its initial volume,the rate of the reaction will become .......
Medium
View SolutionAt $1000 \ K$ 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
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
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