8. For the equilibrium: 2 BrCl (g) Br2 (g) + Cl2 (9) at 205 °C, the equilibrium constant, Kc, is 0.143. If 1.34 moles each of Br2 (g) and Cl2 (g) are introduced in a container which has a volume of 11.0 liters and allowed to reach equilibrium at 205 °C, what would be the concentrations of Br2 (g), Cl2 (g), and BrCl (g) at equilibrium? Ans: [Cl?] = 0.0529 M [Br2] = 0.0529 M [BrCI] = 0.139 M

Question

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2 BrCl (g) ? Br_{2} (g) + Cl_{2} (g)

at

20 5^{?} C

, the equilibrium constant,

Kc

, is 0.143 . If 1.34 moles each of

Br_{2} (g)

and

Cl_{2} (g)

are introduced in a container which has a volume of 11.0 liters and allowed to reach equilibrium at

20 5^{?} C

, what would be the concentrations of

Br_{2} (g), Cl_{2} (g)

, and

BrCl (g)

at equilibrium? Ans:

[Cl_{2}] = 0.0529 M

[Br_{2}] = 0.0529 M [BrCl] = 0.139 M

Accepted Answer

Expert Answer to - 8. For the equilibrium: 2 BrCl (g) Br2 (g) + Cl2 (9) at 205 C, the equilibrium constant, Kc, is 0.

Answer

Solution for - 8. For the equilibrium: 2 BrCl (g) Br2 (g) + Cl2 (9) at 205 C, the equilibrium constant, Kc, is 0.

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This an additional answer to - 8. For the equilibrium: 2 BrCl (g) Br2 (g) + Cl2 (9) at 205 C, the equilibrium constant, Kc, is 0.

(Solved): 8. For the equilibrium: 2 BrCl (g) Br2 (g) + Cl2 (9) at 205 C, the equilibrium constant, Kc, is 0. ...

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