1. Which of the following statements about a system in equilibrium is incorrect?

2. Experimental data was collected for the following reaction.

$1mol$ of each CH4,H2O, and CO are placed in a 1 dm3 container and allowed to equilibrate.
What is the equilibrium concentration of H2​ and CO if there is $0.5mol$ of H2O at equilibrium?

• 	[H2]/mol dm−3	[CO]/mol dm−3
  A.	0.5	0.5
  B.	1.5	0.5
  C.	0.5	1.5
  D.	1.5	1.5

4. Which of the following factors increases the rate of the reaction below?

5. Magnesium and excess hydrochloric acid react together to produce hydrogen gas. This experiment was conducted two times with different hydrochloric acid concentrations but with the same magnesium mass.
In both cases, the volume of hydrogen gas produced was measured at different times, and graphs 1 and 2 were plotted accordingly, as shown below. Choose the letter representing the stage where the rate of reaction is the fastest.

6. If the unit of rate constant, $k$, for a reaction is mol−2 dm6 s−1, what is the overall order of the reaction?

7. The function of the acid-base indicator, In, can be expressed using the equation below

In+H2O ⇋InH++OH−;  Kc=35
Blue    Yellow

Which of the below statements are correct?

I. The solution becomes darker blue with the addition of an acid
II. The solution is a pale green at equilibrium
III.  KcKc​ increases with the addition of an alkali

8. Sodium hydroxide and the ester ethyl acetate react with the rate equation: rate = k[Ester][NaOH].
What are the units of the frequency factor, $A$, for this reaction? k=Ae−Ea/RT

9. Cesium-137 has a half-life of 30 years, and its decay is first order.

How long will it take for a 400$g$ sample to be reduced to 25$g$?

10. A reaction involving X and Y is measured and the following data is found:

What possible mechanism is consistent with the data?

11. A 1 dm3 container contains $2$at equilibrium. What is the value of the equilibrium constant?

12. Reaction 1 has a larger frequency factor, $A$, than reaction 2 but a smaller activation energy, Ea​.
Which of the following graphs is correct?
lnk=−Ea/RT+lnA

13. Two experiments were conducted, and the rates of reactions were measured. In the first experiment, 50 cm^3 of 0.010 mol dm^−3 of sulfuric acid was added to 0.200 g of zinc metal at 25∘∘C. In the second experiment, 50 cm^3 of 0.010 mol dm^−3 of sulfuric acid was added to 0.200 g of zinc metal at 25∘C, followed immediately by 100 cm^3 of distilled water. What happened to reaction rate in the second experiment, and why?

14. In the Arrhenius plot shown below, what is the correct labeling of the x and y axes, respectively?

15. What is the sum of the coefficients when the equation is balanced with whole numbers?

‾ C3H7OH(l)+‾ O2(g)→‾ CO2(g)+‾ H2O(l)​

16. Which change does not affect the position of equilibrium?

17. When pentan-2-one undergoes complete combustion, carbon dioxide and water are the only products. The equation for this reaction is shown.

What are the values of a and b in this equation?

• 	a	b
  A.	7.0	5.0
  B.	7.5	5.0
  C.	8.0	6.0
  D.	8.5	6.0

18. What cannot be used to determine the rate expression for a reaction?

19. Which statements about the equilibrium constant for a reversible reaction are correct?

I. If Kc>>1, the products are favoured
II. If Kc<<1, the reactants are favoured III. If Kc=1, neither products nor reactants are favoured

20. Which graph below represents a second-order reaction?

• A.
• B.
• C.
• D.

21. Which of the following reactions has the largest rate constant, k, under the same reaction conditions?

22. The rate law for the reaction 2 NO(g)+O2(g)→2 NO2(g), is determined to be second-order with respect to $\mathrm{O}$ and first order with respect to O2.
Which of the mixtures below would create the fastest initial rate?

23. Which of the following determines the frequency factor, A, in the Arrhenius equation?

24. What effect would increasing the pressure have on the concentration of H2 and CO2 for the following reaction?

25.