0 of 27 Questions completed
You have already completed the test before. Hence you can not start it again.
Test is loading…
You must sign in or sign up to start the test.
You must first complete the following:
0 of 27 Questions answered correctly
Time has elapsed
You have reached 0 of 0 point(s), (0)
Earned Point(s): 0 of 0, (0)
0 Essay(s) Pending (Possible Point(s): 0)
1. Question1 point(s)Category: K/U
1. A reversible reaction _______.CorrectIncorrect
2. Question1 point(s)Category: K/U
2. Complete the statement below.
Equilibrium happens when _________.CorrectIncorrect
3. Question1 point(s)Category: K/U
3. A system has reached chemical equilibrium. Which is true of the system?CorrectIncorrect
4. Question1 point(s)Category: K/U
4. Which does not remain constant when a system is at dynamic equilibrium?CorrectIncorrect
5. Question1 point(s)Category: K/U
5. Which of these does the equation below represent?
I2(s) ⇔ I2(g)CorrectIncorrect
6. Question1 point(s)Category: K/U
6. Which of the following is not an example of heterogeneous equilibrium?
I. H2O(l) ⇔ H2O(g)
II. C(s) + CO2(g) ⇔ CO2(g)
III. N2O4(g) ⇔ 2NO2(g)
IV. C2H5OH(l) ⇔ C2H5OH(g)
V. CaCO3(s) ⇔ CaO(s) + CO2(g)CorrectIncorrect
7. Question1 point(s)Category: K/U
7. In the equilibrium constant expression below, what do the exponents represent?CorrectIncorrect
8. Question1 point(s)Category: K/U
8. Which is true of the numerical value of the equilibrium constant, Keq?CorrectIncorrect
9. Question1 point(s)Category: K/U
9. Which represents Keq for the equilibrium of the system shown below?
N2(g) + 3H2(g) ⇔ 2NH3(g)
10. Question1 point(s)Category: K/U
10. If a chemical system at equilibrium is disturbed, the rates of the forward and reverse reactions are temporarily unequal. This is known as _____________.CorrectIncorrect
11. Question1 point(s)Category: T
Which is not true regarding the effects temperature changes have on a system at chemical equilibrium?CorrectIncorrect
12. Question1 point(s)Category: T
When a catalyst is added to a chemical system involving a reversible reaction, the catalyst __________.CorrectIncorrect
13. Question1 point(s)Category: T
Which is the correct equation for the quadratic formula?
14. Question1 point(s)Category: T
Which is not true of a reaction quotient?CorrectIncorrect
15. Question1 point(s)Category: T
The following reaction is an example of homogeneous equilibrium:
H2(g) + I2(g) ⇔ 2HI(g)
If the pressure is halved, by doubling the volume and the temperature remains constant, the equilibrium will _______.CorrectIncorrect
16. Question1 point(s)Category: T
A small amount of product is added to the equilibrium system below:
H2(g) + I2(g) ⇔ 2HI(g)
Predict the result.CorrectIncorrect
17. Question1 point(s)Category: T
Nitrogen and oxygen can react as follows:
N2(g) + O2(g) ⇔ 2NO(g) , DH = =180 kJ
If the temperature of the system is increased,CorrectIncorrect
18. Question1 point(s)Category: T
The following systems are at equilibrium.
(i) CO2(g) + 3H2(g) ⇔ CH4(g) + H2O(g)
(ii) H2(g) + I2 (g) ⇔ 2HI(g)
(iii) N2O4(g) ⇔ 2NO2(g)
(iv) N2(g) + 3H2(g) ⇔ 2NH3(g)
Which of the systems will not be affected by a change in pressure?CorrectIncorrect
19. Question1 point(s)Category: T
Phosphorus pentachloride, PCl5(g), undergo decomposition as shown:
PCl5 (g) ⇔ PCl3(g) + Cl2(g)
The equilibrium expression for the reaction is
20. Question1 point(s)Category: T
If the equilibrium shown below is heated at a constant pressure.
H2(g) + I2(g) ⇔ 2HI(g) + 65 kJ
What is most likely to happen?CorrectIncorrect
21. Question2 point(s)Category: C
How does homogeneous equilibrium differ from heterogeneous equilibrium?CorrectIncorrect
22. Question3 point(s)Category: C
Who proposed the Law of Chemical Equilibrium? What is the Law of Mass Action?CorrectIncorrect
23. Question3 point(s)Category: C
An ICE table is useful to organize information about a chemical system. What does the acronym ICE stand for?CorrectIncorrect
24. Question2 point(s)Category: C
Phosphoric acid is found in fertilizers. The exothermic equilibrium reaction used to produce phosphoric acid from water and tetraphosphorus decaoxide is shown below.
P4O10(s) + H2O(l) ⇔ H3PO4(aq) + heat
Based on Le Châtelier’s principle, explain two different ways that you could maximize yields in this equilibrium.CorrectIncorrect
25. Question5 point(s)Category: A
Phosphorous pentachloride is a fine grained powder, ranging in colour from colourless to pale yellow. It has a pungent odour. In the gaseous state it shows the following equilibrium:
PCl5(g) ⇔ PCl3(g) + Cl2(g)
Initially, a sample of phosphorus pentachloride is introduced to an empty vessel. If the equilibrium constant for the above reaction is 4.0 x 10–4 and the equilibrium concentration of [PCl5(g)] is 0.090 mol/L, the equilibrium concentration of [PCl3(g)] is _______ mol/L.CorrectIncorrect
First set up ICE table, then solve for x.
26. Question5 point(s)Category: A
Mountain climbers must take several weeks to get used to the reduced oxygen at high altitudes. The reduced oxygen is a result of the following equilibrium, where Hb represents hemoglobin, the protein that is responsible for transporting oxygen to the cells in the body.
Hb(aq) + O2(g) ⇔ HbO2(g)
a) What happens to the equilibrium when a mountain climber is first introduced to the reduced oxygen?
b) Over time, a mountain climber’s body adjusts by producing more hemoglobin. How does this affect the equilibrium?CorrectIncorrect
27. Question6 point(s)Category: A
In the Haber-Bosch process of manufacturing ammonia, nitrogen is treated with hydrogen, which results in an exothermic reaction. An iron catalyst (Fe3+) is used in the process and aluminum oxide and potassium oxide are used as promoters. The following reactions takes place at 25 oC:
N2(g) + 3H2(g) ⇔ 2NH3(g) + 92 kJ
Indicate the direction in which the equilibrium will shift when:
- temperature is increased.
- volume is increased.
- pressure is decreased.
- a catalyst is added.
- the concentration of N2(g) is increased.
- helium gas is added at constant volume, so that the total pressure is increased.