AP EAPCET 2024 - 21th May Evening Shift | Chemical Equilibrium Question 3 | Chemistry

15 moles of $\mathrm{H}_2$ and 5.2 moles of $\mathrm{I}_2$ are mixed and allowed to attain equilibrium at 773 K . At equilibrium, the number of moles of HI is found to be 10 . The equilibrium constant for the dissociation of HI is

$2 \times 10^{-2}$

$2 \times 10^{-1}$

5.0

AP EAPCET 2024 - 21th May Morning Shift

MCQ (Single Correct Answer)

-0

$K_C$ for the reaction,
$A_2(g) \stackrel{T(\mathrm{~K})}{\rightleftharpoons} B_2(\mathrm{~g})$
is 39.0. In a closed one litre flask, one mole of $A_2(g)$ was heated to $T(\mathrm{~K})$. What are the concentrations of $A_2(g)$ and $B_2(g)$ (in mol L ${ }^{-1}$ ) respectively at equilibrium?

$0.025,0.975$

$0.975,0.025$

$0.05,0.95$

$0.02,0.98$

AP EAPCET 2024 - 20th May Evening Shift

MCQ (Single Correct Answer)

-0

At $T(\mathrm{~K})$, the equilibrium constant for the reaction $\mathrm{H}_2(g)+\mathrm{Br}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HBr}(\mathrm{g})$

is $1.6 \times 10^5$. If 10 bar of HBr is introduced into a sealed vessel at $T(\mathrm{~K})$, the equilibrium pressure of HBr (in bar) is approximately

10.20

10.95

9.95

11.95

AP EAPCET 2024 - 20th May Morning Shift

MCQ (Single Correct Answer)

-0

$K_C$ for the reaction, $A_2(g) \stackrel{T(\mathrm{~K})}{\rightleftharpoons} B_2(g)$ is 99.0 . In a 1 L closed flask two moles of $B_2(g)$ is heated to $T(\mathrm{~K})$. What is the concentration of $B_2(g)\left(\right.$ in $\left.\mathrm{mol} \mathrm{L}^{-1}\right)$ at equilibrium?

0.02

1.98

0.198

1.5

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