The equilibrium constant for the following reaction is1.6\times 10^5 at 1024 K.
$H_{2} (g) + B r_{2} (g) \leftrightarrow 2 H B r (g)$
Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

Q. The equilibrium constant for the reaction is

H_{2} + B r_{2} \to 2 H B r

at 1024 k is

1.60 \times 10^{5} .

Find the equilibrium pressure of all gases if

10 b a r

of HBr is introduced into a sealed container at

1024 K

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A solid XY kept in an evacuated sealed container undergoes decomposition to form a mixture of gases X and Y at temperature T. The equilibrium pressure is 10 bar in this vessel. Kp for this reaction is:

The correct option is A 25XY⇋X(g)+Y(g)At equilibrium, pressure of X and Y will be P(suppose).So, 2P=10;P=5Kp=Px×Py=25

A solid $X Y$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X$ and $Y$ at temperature $T$ . The equilibrium pressure is $10$ bar in this vessel. $K_{p}$ for this reaction is:

The correct option is A $25$
$X Y ⇋ X (g) + Y (g)$
At equilibrium, pressure of $X$ and $Y$ will be $P$ (suppose).
So, $2 P = 10$ ;
$P = 5$
$K_{p} = P_{x} \times P_{y} = 25$