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Standard XII

Chemistry

Cationic Micelle Formation

Bromine monoc...

Question

Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium:

for which K_c= 32 at 500 K. If initially pure BrCl is present at a concentration of 3.3 × 10^–3 molL^–1, what is its molar concentration in the mixture at equilibrium?

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Solution

Let the amount of bromine and chlorine formed at equilibrium be x. The given reaction is:

Now, we can write,

Therefore, at equilibrium,

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Similar questions

Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium:

for which K_c= 32 at 500 K. If initially pure BrCl is present at a concentration of 3.3 × 10^–3 molL^–1, what is its molar concentration in the mixture at equilibrium?

Q. Bromine monochloride,

B r C l

decomposes into bromine and chlorine and reaches the equilibrium.

2 B r C l (g) ⇌ B r_{2} (g) + C l_{2} (g)

;

K_{c} = 32

500 K

. If initially pure

B r C l

is present at a concentration of

3.3 \times 10^{- 3} m o l L^{- 1}

, what is its molar concentration in the mixture at equilibrium?

Q. Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium

2 B r C l (g) \to B r_{2} (g) + C l_{2} (g)

For which

K_{c} = 32

at 500K. If initially pure BrCl is present at a concentration of

3.3 * 10^{- 3} m o l L^{-}

, what is it's molar concentration in the mixture of equilibrium?

Q. Bromine monochloride,

B r C l

, decomposes into bromine and chlorine and reaches equilibrium as

2 B r C l_{(g)} ⇌ B r_{2 (g)} + C l_{2 (g)}

; for which

K_{c} = 32

500 K

If initially, pure

B r C l

is present at a concentration of

3.30 \times 10^{- 3} m o l l i t r e^{- 1}

, what is its molar concentration in the mixture at equilibrium?

Q. (ii) Explain the effect of change of the pressure and temperature in the Haber's process:

2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)} Δ_{r} H^{\circ} = - 193.2 K L .

(iii) Bromine monochloride (BrCl) decomposes into bromine and chlorine and reaches the equilibrium :

2 B r C l_{(g)} ⇌ B r_{2 (g)} + C l_{2 (g)}

.
For which

k c = 32

at 500 K. If initially pure BrCl is present at a concentration of

3.30 \times 10^{- 3} m o l L^{- 1}

what is its molar concentration in the mixture at equilibrium?

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Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium: for which Kc= 32 at 500 K. If initially pure BrCl is present at a concentration of 3.3 × 10–3 molL–1, what is its molar concentration in the mixture at equilibrium?

Let the amount of bromine and chlorine formed at equilibrium be x. The given reaction is: Now, we can write, Therefore, at equilibrium,

Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium:

for which K_c= 32 at 500 K. If initially pure BrCl is present at a concentration of 3.3 × 10^–3 molL^–1, what is its molar concentration in the mixture at equilibrium?

Let the amount of bromine and chlorine formed at equilibrium be x. The given reaction is:

Now, we can write,

Therefore, at equilibrium,