The equilibrium constant for the following reaction is 1-6 - 105 at 1024 K-H 2 g - Br 2 g t-2 HBr g Find the equilibrium pressure of all gases if 10-0 bar of HBr is introduced into a sealed container at 1024 K-

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Standard XII

Chemistry

Equilibrium Constant and Standard Free Energy Change

The equilibri...

Question

The equilibrium constant for the following reaction is 1.6 ×10⁵ at 1024 K.

Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

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Solution

Given,

for the reaction i.e.,

Therefore, for the reaction the equilibrium constant will be,

Now, let p be the pressure of both H₂ and Br₂ at equilibrium.

Now, we can write,

Therefore, at equilibrium,

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Similar questions

The equilibrium constant for the following reaction is 1.6 ×10⁵ at 1024 K.

Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

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 following reactions is

1.6 \times 10^{5}

1024 K

H_{2 (g)} + B r_{2 (g)} ⇌ 2 H B r_{(g)}

Find the equilibrium pressure of all gases if

10.0

bar of

H B r

is introduced into a sealed container at

1024 K

Q. The equilibrium constant for the following reaction is

1.6 \times 10^{5}

at 1024K.

H_{2} (g) + B r_{2} (g) ⇌ 2 H B r (g)

Find the equilibrium pressure of

H_{2}

gas if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

Q. The equilibrium constant for the following reaction is

1.6 \times 10^{5}

1024 K

H_{2} (g) + B r_{2} (g) ⇌ 2 H B r (g)

Find the equilibrium pressure of

H_{2}

gas if

10.0 b a r

H B r

is introduced into a sealed container at

1024 K

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The equilibrium constant for the following reaction is 1.6 ×105 at 1024 K. Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

Given, for the reaction i.e., Therefore, for the reaction the equilibrium constant will be, Now, let p be the pressure of both H2 and Br2 at equilibrium. Now, we can write, Therefore, at equilibrium,

The equilibrium constant for the following reaction is 1.6 ×10⁵ at 1024 K.

Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

Given,

for the reaction i.e.,

Therefore, for the reaction the equilibrium constant will be,

Now, let p be the pressure of both H₂ and Br₂ at equilibrium.

Now, we can write,

Therefore, at equilibrium,