U08CW-KEQ Calc

Write on this assignment.
Respond in complete sentences.
1. What does the chemical equilibrium constant (Keq) predict?
2. Determine whether the following Keq values favor the forward or reverse reaction for reversible
reactions at equilibrium: Keq= 0.85, Keq= 1.00, Keq= 12.00, and Keq= 1.05.
3. Consider the following equilibrium equation.
2SO2 (g) + O2 (g)  2SO3 (g)
Originally, there are equal numbers of moles of SO2 and O2 in a 1.0-liter container. Which of the
following must be true at equilibrium?
a. [SO2] = [SO3]
c. [SO2] = [O2]
e. [SO2] > [O2]
b. 2[SO2] = 2[SO3]
d. [SO2] < [O2]
4. At 985C, the equilibrium constant for the forward reaction below is 1.63. What is the equilibrium
constant for the reverse reaction?
P4 (s) + 6 NO (g)  P4O6 (s) + 3 N2 (g)
Write equilibrium expressions for the following reversible reactions.
5. CH4 (g) + Cl2 (g)  CH3Cl (g) + HCl (g)
6. 2 C2H6 (g) + 7 O2 (g)  4 CO2 (g) + 6 H2O (g)
7. 2 NO (g) + Br2 (g) 2 NOBr (g)
Calculate the Keq for the following systems at equilibrium. Based on the value for Keq, predict the
favored direction.
PROBLEM
Keq CALCULATION
ANSWER
FAVORED
DIRECTION
8. Fe2O3 (s) + 3 H2 (g)  2 Fe (s) + 3 H2O (g)
[Fe2O3] = 0.95 M
[H2] = 0.25 M
[Fe] = 1.50 M
[H2O] = 1.35 M
CaO (s) + CO2 (g)
[CaCO3] = 0.02 M
[CaO] = 0.005 M
[CO2] = 0.0004 M
9. CaCO3
(s)
SC2. Students will relate how the law of conservation of matter is used to determine chemical composition in compounds and chemical
reactions.
f. Explain the role of equilibrium in chemical reactions.
SC5. Students will understand that the rate at which a chemical reaction occurs can be affected by changing concentration, temperature,
or pressure and the addition of a catalyst.
a. Demonstrate the effects of changing concentration, temperature, and pressure on chemical reactions.
 You exceeded the standard(s).
 You met the standard(s).
 You did not meet the standard(s).
Equilibrium Constants
Do not write on this assignment.
10. SnO2 (s) + 2 CO (g) Sn (s) + 2 CO2 (g)
[SnO2] = 0.37 M
[CO] = 0.26 M
[Sn] = 0.33 M
[CO2] = 0.01 M
11. P4 (s) + 6 NO (g)  P4O6 (s) + 3 N2 (g)
[P4] = 1.3 M
[NO] = 0.13 M
[P4O6] = 1.33 M
[N2] = 0.002 M
12. N2 (g) + O2 (g)  2 NO (g)
[N2] = 0.58 M
[O2] = 0.41 M
[NO] = 0.20 M
13. H2 (g) + F2 (g)  2HF (g)
[H2] = 0.61 M
[F2] = 0.18 M
[HF] = 0.87 M
14. 2SO2 (g) + O2 (g)  2SO3 (g)
[SO2] = 1.50 M
[O2] = 1.25 M
[SO3] = 3.50 M
15. 2SO2 (g) + O2 (g)  2SO3 (g)
[SO2] = 0.590 M
[O2] = 0.0445 M
[SO3] = 0.260 M
SC2. Students will relate how the law of conservation of matter is used to determine chemical composition in compounds and chemical
reactions.
f. Explain the role of equilibrium in chemical reactions.
SC5. Students will understand that the rate at which a chemical reaction occurs can be affected by changing concentration, temperature,
or pressure and the addition of a catalyst.
a. Demonstrate the effects of changing concentration, temperature, and pressure on chemical reactions.
 You exceeded the standard(s).
 You met the standard(s).
 You did not meet the standard(s).

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