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Introduction to Le Chatelier's Principle

ctabie11. The...

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ctabie11. The equilibrium constant for the reaction, H2(g) + 12(g)2HI(g)is 32 at a given temperature. The equilibrium concentration of 2 and HI are 0.5 x 10- and8 10-3 M respectively. The equilibrium concentration of H2 is(1) 1 x 10-3 M(2) 0.5 x 10-3 M(4) 4\ast 10-3 M(3) 2x 10-3

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Q. The equilibrium constant for the reaction

H_{2 (g)} + I_{2 (g)} ⇌ 2 {H I}_{(g)}

32

at a given temperature.
The equilibrium concentration of

I_{2}

H I

0.5 \times 10^{- 3} M

8 \times 10^{- 3} M

respectively. The equilibrium concentration of

H_{2}

Q. In the following equilibrium reaction

2 A ⇌ B + C

, the equilibrium concentration of

A, B

C

1 \times 10^{- 3} M, 2 \times 10^{- 3} M

3 \times 10^{- 3} M

respectively at

300 K

Then what is the value of

K_{c}

for this equilibrium reaction at the same temperature?

The equilibrium constant for the given reaction is 81 at a certain temperature. If the concentrations of

H_{2}

I_{2}

are 3 moles/ lit each at equilibrium, the equilibrium concentration of HI is:

H_{2} (g) + I_{2} (g) ⇋ 2 H I (g)

2 H X (g) ⇋ H_{2} (g) + X_{2} (g); K_{C} = 1.0 \times 10^{- 5}

What is the concentration of

H X

if the equilibrium concentration of

H_{2}

X_{2}

1.2 \times 10^{- 3} M

1.2 \times 10^{- 4} M

Q. For the equilibrium system

2 H X (g) ⇌ H_{2} (g) + X_{2} (g)

the equilibrium constant is

1.0 \times 10^{- 5}

. What is the concentration of HX if the equilibrium concentration of

H_{2}

X_{2}

1.2 \times 10^{- 3} M

1.2 \times 10^{- 4} M

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