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When gaseous F2 and solid I2 are heated to high temperatures, the I2 sublimes and gaseous iodine heptafluoride forms. 3.50 × 102 torr of F2 and 4.00 g of solid I2 are put into a 2.50 L container at 2.50 × 102 K and the container is heated to 5.50 × 102 K.

(a) What is the final pressure? Ptotal = atm

(b) What is the partial pressure of I2 gas? PI2 = atm I2

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Related questions

When gaseous F2 and solid I2 are heated high temperatuer the I2 sublimes and gaseous iodine heptofloride forms. 3.40x10^2 torr of F2 and 4.10 g of solid I2 are put in to a 2.5 L container at 2.5x10^2 K and container is heated to 550 K.

What is final pressure.

atm

What is partial pressure of I2 gas.

atm

answer all questions for rating.

1.

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)⇌COCl2(g)

Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 453 ∘C . 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 ∘C :

H2(g)+I2(g)⇌2HI(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?

2.

Part B

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

C(s)+H2O(g)⇌CO(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)⇌C2H2(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)⇌ClF(g)+F2(g).

Calculate the equilibrium partial pressures of ClF3, ClF, and F2 if only ClF3 is present initially, at a partial pressure of 1.59 atm .

± Calculating Equilibrium Constants
The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium.

For a gaseous reaction with the general form

aA+bB⇌cC+dD

the Kc and Kp expressions are given by

Kc=[C]c[D]d[A]a[B]b

Kp=(PC)c(PD)d(PA)a(PB)b

The subscript c or p indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved since their composition does not change throughout the reaction. The standard state of a pure substance is the pure substance itself, and although the quantity may change the sample remain pure. The concentration is effectively equal to 1, and will not impact the magnitude of K.
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)⇌COCl2(g)

Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 456 ∘C . At equilibrium, the concentrations were measured and the following results obtained:

Gas Partial Pressure
(atm)
CO 0.900
Cl2 1.18
COCl2 0.250

What is the equilibrium constant, Kp, of this reaction?
Express your answer numerically.

Kp =
0.235

SubmitHintsMy AnswersGive UpReview Part
Correct
Deriving concentrations from data
In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.
Part B
The following reaction was performed in a sealed vessel at 774 ∘C :

H2(g)+I2(g)⇌2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.10M and[I2]=2.10M. The equilibrium concentration of I2 is 0.0600 M . What is the equilibrium constant, Kc, for the reaction at this temperature?
Express your answer numerically.

Kc =

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