Chemistry 30

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Chemical Equilibrium

Practice Questions 2.1: The Equilibrium Constant
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1.

Write equilibrium expressions for the following reversible reactions:

a. 2 NO2 (g)↔ N2O4 (g)
b. N2 (g) + 3 H2 (g) ↔ 2 NH3 (g)
c. 2 SO2 (g) + O2 (g) ↔ 2 SO3 (g)
2.

For the equilibrium system described by 2 SO2 (g) + O2 (g) ↔ 2 SO3 (g)

at a particular temperature the equilibrium concentrations of SO2, O2 and SO3 were 0.75 M, 0.30 M, and 0.15 M, respectively. At the temperature of the equilibrium mixture, calculate the equilibrium constant, Keq, for the reaction.

3.

For the equilibrium system described by: PCl5 (g) ↔ PCl3 (g) + Cl2 (g)

Keq equals 35 at 487°C. If the concentrations of the PCl5 and PCl3 are 0.015 M and 0.78 M, respectively, what is the concentration of the Cl2?

4.

The following table gives some values for reactant and product equilibrium concentrations (in moles/L; M) at 700 K for the Shift reaction, an important method for the commercial production of hydrogen gas: CO(g) + H2O(g) ↔ CO2 (g) + H2 (g)

Trial
[CO2]
[ H2]
[ CO]
[H2O]
1
0.600
0.600
0.266
0.266
2
0.600
0.800
0.330
0.286
3
2.00
2.00
0.877
0.877
4
1.00
1.50
0.450
0.655
5
1.80
2.00
0.590
1.20

 

Calculate Keq for each of the five trials. How do the answers compare with each other? Why?

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Credits | Central iSchool | Sask Learning | Saskatchewan Evergreen Curriculum | Updated: 27-Jun-2006