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I am Lyosha [343]
3 years ago
14

A mixture of 0.307 M Cl 2 , 0.465 M F 2 , and 0.706 M ClF is enclosed in a vessel and heated to 2500 K . Cl 2 ( g ) + F 2 ( g )

− ⇀ ↽ − 2 ClF ( g ) K c = 20.0 at 2500 K Calculate the equilibrium concentration of each gas at 2500 K .
Chemistry
1 answer:
monitta3 years ago
5 0

<u>Answer:</u> The equilibrium concentration of chlorine gas, fluorine gas and ClF gas is 0.159 M, 0.317 M and 1.002 M respectively.

<u>Explanation:</u>

We are given:

Initial concentration of chlorine gas = 0.307 M

Initial concentration of fluorine gas = 0.465 M

Initial concentration of ClF gas = 0.706 M

The given chemical equation follows:

                            Cl_2(g)+F_2(g)\rightleftharpoons 2ClF(g)

<u>Initial:</u>                  0.307       0.465       0.706

<u>At eqllm:</u>           0.307-x    0.465-x       0.706+2x

The expression of K_c for above equation follows:

K_c=\frac{[ClF]^2}{[Cl_2][F_2]}

We are given:

K_c=20.0

Putting values in above equation, we get:

20.0=\frac{(0.706+2x)^2}{(0.307-x)(0.465-x)}\\\\x=0.148,0.993

Neglecting the value of x = 0.993 because the equilibrium concentrations of chlorine and fluorine gases will become negative, which is not possible

So, equilibrium concentration of chlorine gas = (0.307 - x) = [0.307 - 0.148] = 0.159 M

Equilibrium concentration of fluorine gas = (0.465 - x) = [0.465 - 0.148] = 0.317 M

Equilibrium concentration of ClF gas = (0.706 + 2x) = [0.706 + 2(0.148)] = 1.002 M

Hence, the equilibrium concentration of chlorine gas, fluorine gas and ClF gas is 0.159 M, 0.317 M and 1.002 M respectively.

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<h3>Further explanation</h3>

Given

Molecular formula : C₁₀H₅O₂

Required

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Solution

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