Question

1) The following reaction was carried out in a 2.25 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 8.75 mol of C, 14.1 mol of H2O, 3.60 mol of CO, and 8.50 mol of H2, what is the reaction quotient Q?

2) The following reaction was performed in a sealed vessel at 782 ∘C : H2(g)+I2(g)⇌2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.65M and [I2]=2.65M. The equilibrium concentration of I2 is 0.0900 M . What is the equilibrium constant, Kc, for the reaction at this temperature?

3) A reaction vessel at 27 ∘C contains a mixture of SO2(P= 3.10 atm ) and O2(P= 1.10 atm ). When a catalyst is added the reaction 2SO2(g)+O2(g)⇌2SO3(g) takes place. At equilibrium the total pressure is 3.95 atm . Find the value of Kc.

4) Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.282 Mand [H2S]= 0.370 M . What is the value of the equilibrium constant (Kc) at this temperature? What is Δn for the following equation in relating Kc to Kp?

5) N2(g) + 3 F 2(g) ↔ 2 NF 3(g)

What is Δn for the following equation in relating Kc to Kp?

N2(g) + 3 F 2(g) ↔ 2 NF 3(g)

4
-4
2
1
-2

6) Use the reactions below and their equilibrium constants to predict the equilibrium constant for the reaction, 2A(s)⇌3D(g).
A(s)⇌12B(g)+C(g)K1=0.0334
3D(g)⇌B(g)+2C(g)K2=2.35

Answer 1

1)

th "quotient" Q is given as

Q = [CO][H2]/[H2O]

carbon concentration is ignored since it is a solid; activity = 1

therefore; calculate concnetrations

M = mol/L

n = 14.1 mol of H2O

M = 14.1/2.25 = 6.26666 M of H2O

n = 3.60 mol of CO

M = 3.60 /2.25 = 1.6 M of CO

8.50 mol of H2

M = 8.5/2.25 = 3.777 M of H2

Then

Q = [CO][H2]/[H2O] = (1.6)(3.77)/(6.266) = 0.962655

Q = 0.962655

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