(A) The reaction is $AO_{2(g)} + BO_{2(g)} \rightleftharpoons AO_{3(g)} + BO_{(g)}$.Given $K_c = 16$ and initial concentrations $[AO_2] = [BO_2] = [AO

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(A) The reaction is $AO_{2(g)} + BO_{2(g)} \rightleftharpoons AO_{3(g)} + BO_{(g)}$.Given $K_c = 16$ and initial concentrations $[AO_2] = [BO_2] = [AO_3] = [BO] = 1.0 \ M$.Let the change in concentration be $x$.At equilibrium:$[AO_2] = 1 - x$$[BO_2] = 1 - x$$[AO_3] = 1 + x$$[BO] = 1 + x$$K_c = \frac{[AO_3][BO]}{[AO_2][BO_2]} = \frac{(1+x)(1+x)}{(1-x)(1-x)} = 16$Taking the square root of both sides:$\frac{1+x}{1-x} = 4$$1 + x = 4 - 4x$$5x = 3 \implies x = 0.6$Equilibrium concentration of $[BO] = 1 + x = 1 + 0.6 = 1.6 \ mol \ L^{-1}$.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

Medium

At $T \ K$,$K_c$ for the reaction $AO_{2(g)} + BO_{2(g)} \rightleftharpoons AO_{3(g)} + BO_{(g)}$ is $16$. One mole each of reactants and products are taken in a $1 \ L$ flask and heated to $T \ K$,and equilibrium is established. What is the equilibrium concentration of $BO$ (in $mol \ L^{-1}$)?

TS EAMCET 2024 All TS EAMCET

A
$1.6$
B
$0.4$
C
$1.2$
D
$0.8$

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At $T \ K$,$K_c$ for the reaction $AO_{2(g)} + BO_{2(g)} \rightleftharpoons AO_{3(g)} + BO_{(g)}$ is $16$. One mole each of reactants and products are taken in a $1 \ L$ flask and heated to $T \ K$,and equilibrium is established. What is the equilibrium concentration of $BO$ (in $mol \ L^{-1}$)?

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For the reaction,$2SO_{2(g)} + O_{2(g)} \to 2SO_{3(g)}$$\Delta H = -57.2 \ kJ \ mol^{-1}$ and $K_C = 1.7 \times 10^{16}$Which of the following statement is $INCORRECT$?

Which one of the following statements is correct for a reversible reaction? $A$ catalyst

For the reaction $A + B \rightleftharpoons C + D$ at $250^\circ C$ in a $1 \ L$ vessel,the initial concentration of $A$ is $3$ and $B$ is $n$. If the equilibrium concentration of $C$ is equal to the equilibrium concentration of $B$,what is the equilibrium concentration of $D$?

The following reaction is performed at $298 \, K$.$2 NO_{(g)} + O_{2(g)} \rightleftharpoons 2 NO_{2(g)}$The standard free energy of formation of $NO_{(g)}$ is $86.6 \, kJ/mol$ at $298 \, K$. What is the standard free energy of formation of $NO_{2(g)}$ at $298 \, K$? $(K_p = 1.6 \times 10^{12})$

For the equilibrium reaction $A + B \rightleftharpoons C + D$,if we start with equal concentrations of $A$ and $B$,at equilibrium,the concentration of $C$ is $2$ times that of $A$. Find the value of $K_c$.

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For the reaction,$2SO_{2(g)} + O_{2(g)} \to 2SO_{3(g)}$
$\Delta H = -57.2 \ kJ \ mol^{-1}$ and $K_C = 1.7 \times 10^{16}$
Which of the following statement is $INCORRECT$?

The following reaction is performed at $298 \, K$.
$2 NO_{(g)} + O_{2(g)} \rightleftharpoons 2 NO_{2(g)}$
The standard free energy of formation of $NO_{(g)}$ is $86.6 \, kJ/mol$ at $298 \, K$. What is the standard free energy of formation of $NO_{2(g)}$ at $298 \, K$? $(K_p = 1.6 \times 10^{12})$