0%

SL - How much, how fast and how far

25 MCQ from 2025 Question Bank How much, how fast and how far(all topics)

DP IB SL Chemistry Quiz

 

1 / 25

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

H2O(g)+CO(g)⇌H2(g)+CO2(g)

2 / 25

2. What do you call the maximum amount of product that would result from the complete consumption of the limiting reagent?

 

3 / 25

3. What is the equilibrium constant expression for the reaction below?

2 HCl(g)⇌H2(g)+Cl2(g)

4 / 25

4. 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.   increases with the addition of an alkali

5 / 25

5. Two experiments were conducted, and the rates of reaction were measured. In the first experiment, 50 cm^3 of 0.010 mol dm^− of sulfuric acid was added to 0.200 g of zinc metal at 25 °C. In the second experiment, 50 cm of 0.010 mol dm− 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 the reaction rate in the second experiment, and why?

6 / 25

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

 

7 / 25

7. Which row of the table correctly states the changes that occur when the temperature is increased for the following reaction:

PbO2(s)⇌PbO(s)+1/2O2(g) ΔH=+ve

  • Value of the equilibrium constant Position of equilibrium
    A. Changes Shifts towards the products
    B. Changes Shifts towards the reactants
    C. Stays the same Shifts towards the products
    D. Stays the same Shifts towards the reactants

8 / 25

8. 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.

6.1-327

9 / 25

9.

10 / 25

10. Nitrogen gas reacts with hydrogen gas to produce ammonia as per the following chemical equation:

N2(g)+3H2(g)→2NH3(g)

If 0.86  of N2 are mixed with 0.50  of H2, which reactant is in excess?

11 / 25

11.

12 / 25

12. Propane gas is combusted in oxygen gas according to the following equation:

C3H8(g)+5O2(g)→3CO2(g)+4 H2O(g)

When 11.0 g of propane gas (MW 44.097) is combusted in 8.0 g of oxygen gas, 0.20 moles of water vapor is produced.
What is the excess reactant and how many moles remain after the reaction is complete?

13 / 25

13. A 1 dm3 container contains 2 mol NH3,1 mol N2 and 1 mol H2 at equilibrium. What is the value of the equilibrium constant?

N2+3 H2⇌2 NH3

14 / 25

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

Mg(s) + 2HNO3(aq) → Mg(NO)2(aq) + H2(g)

15 / 25

15. The following graph represents the change of concentration of a gaseous reactant and gaseous product during a reaction. At t=10 mins, the temperature is increased and at t=15 mins, the volume of the reaction vessel is increased.

7.1-81

Which row of the table below correctly describes the enthalpy change of the forward reaction and the moles of gas of the reactants and products?

  • Enthalpy change of forward reaction Moles of gas
    A. Exothermic Reactants more than the products
    B. Exothermic Reactants less than the products
    C. Endothermic  Reactants more than the products
    D. Endothermic Reactants less than the products

16 / 25

16. 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

17 / 25

17. Which conditions would increase the equilibrium yield of H?

CH4 (g)+H2O (g) ⇋CO (g)+3H2 (g)  ΔH=+210 kJ

  • I. Increase the volume of the reaction vessel
  • II. Increase the temperature
  • III. Use a catalyst

18 / 25

18. When balanced, what is the sum of the correct coefficients for the following reaction?

__ LiOH (aq)^+ __ H2SO (aq) → __ LiSO(aq)^+ __HO (l)

19 / 25

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

20 / 25

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

Pentan-2-one+a O2 →b CO2+b H2O

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

21 / 25

21. Which statement(s) are correct for the below system at dynamic equilibrium?

KI (s) ⇋K+ (aq)+I−  (aq)

  • I. KI was initially added to the water in excess
  • II. No matter is exchanged with the surroundings
  • III. The rate of dissolution is equal to the rate of precipitation

22 / 25

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

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

23 / 25

23.

24 / 25

24. The Maxwell-Boltzmann distribution plot below is for the same substance with the same concentration at different temperatures. Which statement is correct about the total number of molecules for each temperature?

6.1-326

25 / 25

25. Yellow chromate ions CrO42−, and orange dichromate ions Cr2O72−, are in equilibrium according to the following reaction:

2CrO4^2−(aq)+2 H^+(aq)⇌Cr2O7^2−(aq)+H2O (l) 

What will happen if OH^ ions are added to the reaction vessel?

Your score is

0%