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Standard XII

Chemistry

Reaction Quotient

At 700 K, equ...

Question

At 700 K, equilibrium constant for the reaction

is 54.8. If 0.5 molL^–1 of HI₍_g₎ is present at equilibrium at 700 K, what are the concentration of H₂₍_g₎ and I₂₍_g₎ assuming that we initially started with HI₍_g₎ and allowed it to reach equilibrium at 700 K?

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Solution

It is given that equilibrium constantfor the reaction

is 54.8.

Therefore, at equilibrium, the equilibrium constant for the reaction

will be .

Let the concentrations of hydrogen and iodine at equilibrium be x molL^–1

.

Hence, at equilibrium,

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Similar questions

At 700 K, equilibrium constant for the reaction

is 54.8. If 0.5 molL^–1 of HI₍_g₎ is present at equilibrium at 700 K, what are the concentration of H₂₍_g₎ and I₂₍_g₎ assuming that we initially started with HI₍_g₎ and allowed it to reach equilibrium at 700 K?

Q. At

700 K

, the equilibrium constant for the reaction;

H_{2 (g)} + I_{2 (g)} ⇌ 2 H I_{(g)}

54.8

0.5 m o l l i t r e^{- 1}

H I_{(g)}

is present at equilibrium at

700 K

, what are the concentrations of

H_{2 (g)}

and

I_{2 (g)}

assuming that we initially started with

H I_{(g)}

and allowed it to reach equilibrium at

700 K

Q. At

700 K

, equilibrium constant for the reaction:

H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)

64

. If

0.5 m o l

L^{- 1}

H I (g)

is present at equilibrium at

700 K

, what are the concentration of

H_{2} (g)

and

I_{2} (g)

assuming that we initially started with

H I (g)

and allowed it to reach equilibrium at

700 K

Q. At 700 K, equilibrium constant for the reaction:

H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)

is 64. If

0.5 m o l L^{- 1}

of HI(g) is present at equilibrium at 700 K, what are the concentration of

H_{2} (g)

and

I_{2} (g)

assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K?

Q. At

500

K, the equilibrium constant for the reaction

H_{2 (g)} + I_{2 (g)} ⇌ 2 H I_{(} g) i s 24.8

. If

\frac{1}{2} m o l / L

of HI is present at equilibrium. What are the concentrations of

H_{2}

and

I_{2}

, assuming that we started by taking HI and reached the equilibrium at

500

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At 700 K, equilibrium constant for the reaction is 54.8. If 0.5 molL–1 of HI(g) is present at equilibrium at 700 K, what are the concentration of H2(g) and I2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K?

It is given that equilibrium constantfor the reaction is 54.8. Therefore, at equilibrium, the equilibrium constant for the reaction will be . Let the concentrations of hydrogen and iodine at equilibrium be x molL–1 . Hence, at equilibrium,

At 700 K, equilibrium constant for the reaction

is 54.8. If 0.5 molL^–1 of HI₍_g₎ is present at equilibrium at 700 K, what are the concentration of H₂₍_g₎ and I₂₍_g₎ assuming that we initially started with HI₍_g₎ and allowed it to reach equilibrium at 700 K?

It is given that equilibrium constantfor the reaction

is 54.8.

Therefore, at equilibrium, the equilibrium constant for the reaction

will be .

Let the concentrations of hydrogen and iodine at equilibrium be x molL^–1

.

Hence, at equilibrium,