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whitebat914Lv1

21 Mar 2020

At 100 °C, the equilibrium constant for the reaction COCl₂(g) CO(g) + Cl₂(g) has the value K_c = 2.19 × 10^–10. Are the following mixtures of COCl₂, CO, and Cl₂ at
100 °C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium.
(a) [COCl₂] = 2.00 × 10^-3 M, [CO] = 3.3 × 10^-6 M, [Cl₂] = 6.62 × 10^-6 M
(b) [COCl₂] = 4.50 × 10^-2 M, [CO] = 1.1 × 10^-7 M, [Cl₂] = 2.25 × 10^-6 M
(c) [COCl₂] = 0.0100 M, [CO] = [Cl₂] = 1.48 × 10^-6 M

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Lelia LubowitzLv2

13 May 2020

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Consider the following system at equilibrium where HÂ° = -108 kJ, and Kc = 77.5, at 600 K. CO(g) + Cl2(g) COCl2(g)

If the VOLUME of the equilibrium system is suddenly decreased at constant temperature:

The value of Kc:

A. increases. B. decreases. C. remains the same.

The value of Qc:

A. is greater than Kc. B. is equal to Kc. C. is less than Kc.

The reaction must:
A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium.

The number of moles of Cl2 will:

A. increase. B. decrease. C. remain the same.

answer all questions for rating.

Part A

Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures:

CO(g)+Cl2(g)âCOCl2(g)

Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 453 âC . At equilibrium, the concentrations were measured and the following results obtained:

Gas	Partial Pressure (atm)
CO	0.800
Cl2	1.24
COCl2	0.240

What is the equilibrium constant, Kp, of this reaction?

Part B

The following reaction was performed in a sealed vessel at 737 âC :

H2(g)+I2(g)â2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.10M and [I2]=2.35M. The equilibrium concentration of I2 is 0.0100 M . What is the equilibrium constant, Kc, for the reaction at this temperature?

Part B

The following reaction was carried out in a 3.25 L reaction vessel at 1100 K:

C(s)+H2O(g)âCO(g)+H2(g)

If during the course of the reaction, the vessel is found to contain 8.00 mol of C, 14.4 mol of H2O, 3.90 mol of CO, and 6.10 mol of H2, what is the reaction quotient Q?

Part C

The reaction

2CH4(g)âC2H2(g)+3H2(g)

has an equilibrium constant of K = 0.154.

If 6.60 mol of CH4, 4.10 mol of C2H2, and 11.50 mol of H2 are added to a reaction vessel with a volume of 5.80 L , what net reaction will occur?

The reaction

has an equilibrium constant of = 0.154.

If 6.60 of , 4.10 of , and 11.50 of are added to a reaction vessel with a volume of 5.80 , what net reaction will occur?

The reaction will proceed to the left to establish equilibrium.

The reaction will proceed to the right to establish equilibrium.

No further reaction will occur because the reaction is at equilibrium.

3. At 700 K, Kp = 0.140 for the reaction ClF3(g)âClF(g)+F2(g).