COMEDK 2025 Afternoon Shift | Chemical Equilibrium Question 1 | Chemistry

For the reaction $\mathrm{P}+\mathrm{Q} \leq \mathrm{R}+\mathrm{S}$, carried out at 298 K , the equilibrium constant was found to be 169 and the initial concentrations of all reactants and products was 1.0 M . What is the equilibrium concentration of the reactants?

0.143 M

0.462 M

0.857 M

0.698 M

COMEDK 2024 Evening Shift

MCQ (Single Correct Answer)

-0

At $$700 \mathrm{~K}$$, the Equilibrium constant value for the formation of $$\mathrm{HI}$$ from $$\mathrm{H}_2$$ and $$\mathrm{I}_2$$ is 49.0 . 0.7 mole of $$\mathrm{HI}(\mathrm{g})$$ is present at equilibrium. What will be the concentrations of $$\mathrm{H}_2$$ and $$\mathrm{I}_2$$ gases if we initially started with $$\mathrm{HI}(\mathrm{g})$$ and allowed the reaction to reach equilibrium at the same temperature?

0.1195

0.3442

0.4692

0.521

COMEDK 2024 Afternoon Shift

MCQ (Single Correct Answer)

-0

$$\mathrm{S}_8$$ on heating at a temperature above $$1000 \mathrm{~K}$$, changes to $$\mathrm{S}_2$$. When 1 mole of $$\mathrm{S}_8$$ is heated above $$1000 \mathrm{~K}$$, the pressure falls by $$32 \%$$ at equilibrium. The equilibrium constant for the conversion is:

$$4.50 \mathrm{~atm}^3$$

$$2.55 \mathrm{~atm}^3$$

$$3.20 \mathrm{~atm}^3$$

$$3.94 \mathrm{~atm}^3$$

COMEDK 2023 Morning Shift

MCQ (Single Correct Answer)

-0

Consider the following equilibrium,

$$\begin{aligned} & 2 \mathrm{No}(g) \rightleftharpoons \mathrm{N}_2+\mathrm{O}_2 ; \mathrm{K}_{\mathrm{G}}=2.4 \times 10^{20} \\ & \mathrm{No}(\mathrm{g})+\frac{1}{2} \mathrm{Br}_2(\mathrm{~g}) \rightleftharpoons \mathrm{NoBr}(\mathrm{g}) ; \mathrm{K}_{\mathrm{C}_2}=1.4 \end{aligned}$$

Calculate $$K_C$$ for the reaction,

$$\frac{1}{2} \mathrm{~N}_2(g)+\frac{1}{2} \mathrm{O}_2(g)+\frac{1}{2} \mathrm{Br}_2(g) \rightleftharpoons \mathrm{NOBr}(g)$$

$$8.96 \times 10^{-11}$$

$$9.48 \times 10^{-9}$$

$$8.08 \times 10^{-12}$$

$$8.96 \times 10^{11}$$

COMEDK Subjects