Class 11Chemistry6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)
MediumIn the reaction $CH_3COOH + C_2H_5OH \rightleftharpoons CH_3COOC_2H_5 + H_2O$,one mole of each of acetic acid and ethanol is heated in the presence of a little concentrated $H_2SO_4$. When equilibrium is reached,which of the following is true?
- A$1$ mole of ethyl acetate is produced
- B$2$ moles of ethyl acetate are produced
- C$2/3$ mole of ethyl acetate is produced
- DThe amount cannot be predicted
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Similar Questions
Calculate:
$(a)$ $\Delta G^{\circ}$ and
$(b)$ the equilibrium constant for the formation of $NO_2$ from $NO$ and $O_2$ at $298 \, K$
$NO_{(g)} + 1/2 O_{2(g)} \longleftrightarrow NO_{2(g)}$
Given:
$\Delta G^{\circ}_f(NO_2) = 52.0 \, kJ/mol$
$\Delta G^{\circ}_f(NO) = 87.0 \, kJ/mol$
$\Delta G^{\circ}_f(O_2) = 0 \, kJ/mol$
$(a)$ $\Delta G^{\circ}$ and
$(b)$ the equilibrium constant for the formation of $NO_2$ from $NO$ and $O_2$ at $298 \, K$
$NO_{(g)} + 1/2 O_{2(g)} \longleftrightarrow NO_{2(g)}$
Given:
$\Delta G^{\circ}_f(NO_2) = 52.0 \, kJ/mol$
$\Delta G^{\circ}_f(NO) = 87.0 \, kJ/mol$
$\Delta G^{\circ}_f(O_2) = 0 \, kJ/mol$
Medium
View SolutionAt high temperature,$2 \, \text{mol}$ of $NH_3$ is placed in a $500 \, \text{mL}$ vessel. For the decomposition reaction $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$,if $1 \, \text{mol}$ of $NH_3$ remains at equilibrium,then $K_c$ is equal to:
Medium
View SolutionFor the following reaction,the equilibrium constant $K_{c}$ at $298 \ K$ is $1.6 \times 10^{17}$.
$Fe^{2+}_{(aq)} + S^{2-}_{(aq)} \rightleftharpoons FeS_{(s)}$
When equal volumes of $0.06 \ M \ Fe^{2+}_{(aq)}$ and $0.2 \ M \ S^{2-}_{(aq)}$ solutions are mixed,the equilibrium concentration of $Fe^{2+}_{(aq)}$ is found to be $Y \times 10^{-17} \ M$. The value of $Y$ is. . . . .
$Fe^{2+}_{(aq)} + S^{2-}_{(aq)} \rightleftharpoons FeS_{(s)}$
When equal volumes of $0.06 \ M \ Fe^{2+}_{(aq)}$ and $0.2 \ M \ S^{2-}_{(aq)}$ solutions are mixed,the equilibrium concentration of $Fe^{2+}_{(aq)}$ is found to be $Y \times 10^{-17} \ M$. The value of $Y$ is. . . . .
MediumIIT 2019
View SolutionThe equilibrium constants of the following are
$N_2 + 3H_2 \rightleftharpoons 2NH_3 \,; \quad K_1$
$N_2 + O_2 \rightleftharpoons 2NO \,; \quad K_2$
$H_2 + \frac{1}{2} O_2 \rightleftharpoons H_2O \,; \quad K_3$
The equilibrium constant $(K)$ of the reaction:
$2NH_3 + \frac{5}{2} O_2 \rightleftharpoons 2NO + 3H_2O$ is:
$N_2 + 3H_2 \rightleftharpoons 2NH_3 \,; \quad K_1$
$N_2 + O_2 \rightleftharpoons 2NO \,; \quad K_2$
$H_2 + \frac{1}{2} O_2 \rightleftharpoons H_2O \,; \quad K_3$
The equilibrium constant $(K)$ of the reaction:
$2NH_3 + \frac{5}{2} O_2 \rightleftharpoons 2NO + 3H_2O$ is:
DifficultAIPMT 2007
View Solution$3.00 \, mol$ of $PCl_5$ kept in $1 \, L$ closed reaction vessel was allowed to attain equilibrium at $380 \, K$. Calculate the composition of the mixture at equilibrium. Given $K_c = 1.80$.
Medium
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