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1. The equilibrium constant K for the reaction 2H2S(g) → 2H2(g) + S2(g) is calculated to be 2.25 x 10-2 based on the amounts of reactants and products provided in a 10 L container heated to 1132°C. 2. For the reaction 2NO(g) + O2(g) → 2NO2(g), the equilibrium concentration of NO2 is calculated to be 1.8 x 10-2 mol/L given K = 4.0 x 1013 at 25°C and the initial concentrations of NO and O2 provided. 3. The chemical equation that generates the equilibrium expression K = [CS

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103 views2 pages

More Eq Questions Answers

1. The equilibrium constant K for the reaction 2H2S(g) → 2H2(g) + S2(g) is calculated to be 2.25 x 10-2 based on the amounts of reactants and products provided in a 10 L container heated to 1132°C. 2. For the reaction 2NO(g) + O2(g) → 2NO2(g), the equilibrium concentration of NO2 is calculated to be 1.8 x 10-2 mol/L given K = 4.0 x 1013 at 25°C and the initial concentrations of NO and O2 provided. 3. The chemical equation that generates the equilibrium expression K = [CS

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kimmo
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More Equilibrium Constant Practice

1. When 0.100 mol of hydrogen sulfide was placed in a 10.0 L container and heated
to 1132˚C, it produced an equilibrium mixture that contained 0.0285 mol of
hydrogen. What is K at this temperature?

2H2S(g)  2H2(g) + S2(g)

K = 2.25 x 10-2

2. K for the following reaction is 4.0 x 1013 at 25˚C. If the equilibrium


concentrations of nitrogen monoxide and oxygen gases each were
2.0 x 10-6 mol/L, what is the equilibrium concentration of the nitrogen dioxide?

2NO(g) + O2(g)  2NO2(g)

[NO2] = 1.8 x 10-2 mol/L

3. What gaseous chemical equation generated this equilibrium law expression?

K = [CS2] [H2]4
[CH4] [H2S]2

CH4(g) + 2 H2S(g) ↔ CS2(g) + 4 H2(g)

4. A 5.00 L vessel contains 0.0185 mol of phosphorus trichloride, 0.0158 mol of


phosphorus pentachloride and 0.0870 mol of chlorine gases at 230˚C in
equilibrium. Calculate K.

PCl3(g) + Cl2(g)  PCl5(g)

K = 49.1

5. A gaseous one litre equilibrium mixture of 0.012 mol of carbon monoxide and
0.025 mol of chlorine are found, along with phosgene, COCl2(g). If the K at this
temperature is 1230, what is the equilibrium concentration of phosgene?

You cannot solve this without the reaction. While you know the identities of all
species, you do not know which species are reactants and which are products.

6. What are the equilibrium concentrations of all species when gaseous iodine
bromide is formed from gaseous elements at 150˚C? Initially, there were 0.0015
mol of each element in a 5.0 L vessel, and K at this temperature is 120.

[I2]eq = [Br2]eq = 4.6 x 10-5 mol/L [IBr]eq = 5.1 x 10-4 mol/L


7. The equilibrium constant for a reaction is 9.1 x 10-4 at a temperature. What are the
equilibrium concentrations of all species, if initially the concentration of FeSCN2+
is 2.0 mol/L?

FeSCN2+(aq)  Fe3+ (aq) + SCN1=(aq)

[Fe3+]eq = [SCN1+]eq = 4.3 x 10-2 mol/L [FeSCN2+ ]eq = 2.0 mol/L

8. For the following reaction, K = 9.30 x 10-8 at 700C. When a 3.00 L flask is used,
and 0.46 mol of H2 and 0.30 mol of S2 are present in the flask initially, what
equilibrium concentrations will exist for all species at some later time?

2H2S(g)  2H2(g) + S2(g)

[H2S]eq = 4.7 x 10-5 mol/L [H2]eq = 3.1 x 10-4 mol/L [S2]eq = 2.3 x 10-2 mol/L

9. 2SO2(g) + O2(g) ↔ 2SO3(g) K = 287

Assuming the temperature remains a constant, calculate K when the reaction:


a. coefficients are halved. (K2) K = 16.9
b. is reversed (1/K) K = 3.48 x 10-3
c. reaction is reversed and the coefficients are halved (1/K½) K = 5.90 x 10-2
d. reaction coefficients are doubled. (K2) K = 8.24 x 104

10. No calculator!!!! At 400ºC, a 3.00 L flask contains 3.50 mol HI(g), 4.10 mol of
H2(g), and 0.30 mol of I2(g) in equilibrium. K = ?

H2(g) + I2(g) ↔ 2HI(g)

Approximately 10

11. No calculator again!!!! A 2.0 L flask contains 2.0 mol of hydrogen sulfide gas,
0.40 mol of hydrogen gas, and 0.80 mol of sulfur gas at equilibrium at 450ºC.
What is K?

2H2(g) + S2(g)  2H2S(g)


Approximately 50

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