Difficult
Explain the calculation of equilibrium concentrations given the value of the equilibrium constant.
(N/A) To calculate equilibrium concentrations when initial concentrations are known and the equilibrium constant $(K_c)$ is provided,follow these steps:
Step-$1$: Write the balanced chemical equation for the reaction.
Step-$2$: Create an $ICE$ (Initial,Change,Equilibrium) table under the balanced equation for each substance involved.
$(i)$ List the initial concentration.
$(ii)$ Define the change in concentration as $x$ (in $mol/L$) based on the stoichiometry of the reaction.
$(iii)$ Express the equilibrium concentration as the sum of the initial concentration and the change.
Step-$3$: Substitute these equilibrium concentrations into the equilibrium constant expression $(K_c)$ and solve the resulting algebraic equation for $x$. If a quadratic equation is obtained,select the root that is physically meaningful (i.e.,concentrations must be positive).
Step-$4$: Use the calculated value of $x$ to determine the actual equilibrium concentrations of all reactants and products.
Step-$5$: Verify the results by substituting the calculated equilibrium concentrations back into the $K_c$ expression to ensure they yield the given constant.
Step-$1$: Write the balanced chemical equation for the reaction.
Step-$2$: Create an $ICE$ (Initial,Change,Equilibrium) table under the balanced equation for each substance involved.
$(i)$ List the initial concentration.
$(ii)$ Define the change in concentration as $x$ (in $mol/L$) based on the stoichiometry of the reaction.
$(iii)$ Express the equilibrium concentration as the sum of the initial concentration and the change.
Step-$3$: Substitute these equilibrium concentrations into the equilibrium constant expression $(K_c)$ and solve the resulting algebraic equation for $x$. If a quadratic equation is obtained,select the root that is physically meaningful (i.e.,concentrations must be positive).
Step-$4$: Use the calculated value of $x$ to determine the actual equilibrium concentrations of all reactants and products.
Step-$5$: Verify the results by substituting the calculated equilibrium concentrations back into the $K_c$ expression to ensure they yield the given constant.
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Similar Questions
For the following three reactions $a, b$ and $c,$ equilibrium constants are given:
$(i)$ $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$ ; $K_1$
$(ii)$ $CH_{4(g)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + 3H_{2(g)}$ ; $K_2$
$(iii)$ $CH_{4(g)} + 2H_2O_{(g)} \rightleftharpoons CO_{2(g)} + 4H_{2(g)}$ ; $K_3$
Which of the following relations is correct?
$(i)$ $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$ ; $K_1$
$(ii)$ $CH_{4(g)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + 3H_{2(g)}$ ; $K_2$
$(iii)$ $CH_{4(g)} + 2H_2O_{(g)} \rightleftharpoons CO_{2(g)} + 4H_{2(g)}$ ; $K_3$
Which of the following relations is correct?
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View SolutionIf for ${H_2(g)} + \frac{1}{2}{S_2(s)} \rightleftharpoons {H_2S(g)}$ and ${H_2(g)} + {Br_2(g)} \rightleftharpoons 2{HBr(g)}$ the equilibrium constants are $K_1$ and $K_2$ respectively,the reaction ${Br_2(g)} + {H_2S(g)} \rightleftharpoons 2{HBr(g)} + \frac{1}{2}{S_2(s)}$ would have equilibrium constant
Difficult
View Solution$K_{a_1}, K_{a_2}$ and $K_{a_3}$ are the respective ionization constants for the following reactions $(a), (b),$ and $(c)$.
$(a)$ $H_2C_2O_4 \rightleftharpoons H^{+} + HC_2O_4^-$
$(b)$ $HC_2O_4^- \rightleftharpoons H^{+} + C_2O_4^{2-}$
$(c)$ $H_2C_2O_4 \rightleftharpoons 2H^{+} + C_2O_4^{2-}$
The relationship between $K_{a_1}, K_{a_2}$ and $K_{a_3}$ is given as
$(a)$ $H_2C_2O_4 \rightleftharpoons H^{+} + HC_2O_4^-$
$(b)$ $HC_2O_4^- \rightleftharpoons H^{+} + C_2O_4^{2-}$
$(c)$ $H_2C_2O_4 \rightleftharpoons 2H^{+} + C_2O_4^{2-}$
The relationship between $K_{a_1}, K_{a_2}$ and $K_{a_3}$ is given as
DifficultJEE MAIN 2022
View SolutionFor the reversible reaction $2HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)}$, the unit of the equilibrium constant $K_c$ is:
Easy
View SolutionWrite the equilibrium constant (equilibrium law) for the following reactions:
$(i)$ $4NH_{3(g)} + 5O_{2(g)} \rightleftharpoons 4NO_{(g)} + 6H_{2}O_{(g)}$
$(ii)$ $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$
$(iii)$ $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
$(i)$ $4NH_{3(g)} + 5O_{2(g)} \rightleftharpoons 4NO_{(g)} + 6H_{2}O_{(g)}$
$(ii)$ $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$
$(iii)$ $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
Medium
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