Name:_________________________________ Date:________________Kinetics and Equilibrium 2018 Mrs. Mannion

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A) proper orientation, onlyB) both proper energy and proper orientationC) neither proper energy nor proper orientationD) proper energy, only

1. A reaction is most likely to occur when reactantparticles collide with

A) ionization energyB) activation energyC) heat of reactionD) heat of vaporization

2. After being ignited in a Bunsen burner flame, a pieceof magnesium ribbon burns brightly, giving off heatand light. In this situation, the Bunsen burner flameprovides

A) NaOH B) NaClC) NH4Cl D) LiBr

3. At 101.3 kPa and 298 K, a 1.0-mole sample of whichcompound absorbs the greatest amount of heat as theentire sample dissolves in water?

A) concentration B) volumeC) heat of reaction D) activation energy

4. If the pressure on gaseous reactants is increased, therate of reaction is increased because there is anincrease in the

A) more contact with the H+ ions in the acidB) less contact with the H+ ions in the acidC) lower average kinetic energyD) higher average kinetic energy

5. A 1.0-gram sample of powdered Zn reacts faster withHCl than a single 1.0-gram piece of Zn because theatoms in powdered Zn have

A) Only the rate of the reverse reaction will beincreased.

B) The energy change ( H) of the reaction will bedecreased.

C) The activation energy will be changed.D) Only the rate of the forward reaction will be

increased.

6. Which will occur if a catalyst is added to a reactionmixture?

A) endothermic B) spontaneousC) redox D) exothermic

7. In what type of reaction do the products of thereaction always possess more potential energy thanthe reactants?

A) 89 kJ of energy is absorbed and the temperatureof the water decreases

B) 89 kJ of energy is released and thetemperature of the water increases

C) 44.5 kJ of energy is absorbed and thetemperature of the water decreases

D) 44.5 kJ of energy is released and the temperatureof the water increases

8. Based on Reference Table I, when 2.00 moles ofNaOH(s) dissolves in water

A) B)C) D)

9. Given the reaction:

What is the heat of formation of nitrogen (II) oxide inkJ/mole?

A) 2 B) 1 C) 4 D) 3

10. Given the potential energy diagram for a reaction:

Which interval on this diagram represents thedifference between the potential energy of theproducts and the potential energy of the reactants?

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A) B + D B) A + BC) B + C D) C + D

11. Given the potential energy diagram representing areversible reaction:

The activation energy for the reverse reaction isrepresented by

A) 1 and 3 B) 3 and 4C) 2 and 3 D) 1 and 2

12. The potential energy diagram below shows thereaction

X + Y Z.

When a catalyst is added to the reaction, it willchange the value of

A) A B) B C) C D) D

13. In the potential energy diagram below, which letterrepresents the potential energy of the activatedcomplex?

A) increasesB) remains the sameC) increasesD) remains the same

14. Given the equation for a system at equilibrium:

If only the concentration of is increased, theconcentration of

A) rate at which products are formed is thesame as the rate at which reactants areformed

B) concentration of products is the same as theconcentration of reactants

C) concentration of products is greater than theconcentration of reactants

D) rate at which products are formed is greaterthan the rate at which reactants are formed

15. A system is said to be in a state of dynamicequilibrium when the

A) 298 K B) 100 KC) 373 K D) 273 K

16. Given the equilibrium at 101.3 kPa:

H2O(s) « H2O( )

At what temperature does this equilibrium occur?

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A) decrease B) increaseC) remain the same

17. Given the reaction at equilibrium:

N2(g) + O2(g) = 2 NO(g)

If the temperature remains constant and the pressureincreases, the number of moles of NO(g) will

A) increasing the pressureB) adding more A(g)C) increasing the temperatureD) adding a catalyst

18. Given the reaction at equilibrium:

2 A(g) + 3 B(g) « A2B3(g) + heat

Which change will not affect the equilibriumconcentrations of A(g), B(g), and A2B3(g)?

A) increasing the concentration of B) decreasing the pressureC) decreasing the concentration of D) increasing the temperature

19. Given the equation representing a reaction atequilibrium:

Which change causes the equilibrium to shift to theright?

A) The equilibrium will shift to the right and[HI] will increase.

B) The equilibrium will shift to the right and [HI]will decrease.

C) The equilibrium will shift to the left and [H2]will decrease.

D) The equilibrium will shift to the left and [H2]will increase.

20. Given the equilibrium reaction in a closed system:

H2(g) + I2(g) + heat 2 HI(g)What will be the result of an increase intemperature?

A) an exothermic reaction in which entropydecreases

B) an endothermic reaction in which entropyincreases

C) an endothermic reaction in which entropydecreases

D) an exothermic reaction in which entropyincreases

21. Which chemical reaction will always bespontaneous?

A) B)

C) D)

22. Each of four test tubes contains a differentconcentration of HCI(aq) at 25°C. A 1-gram cube ofZn is added to each test tube. In which test tube isthe reaction occurring at the fastest rate?

23. Base your answer to the following question on thetable below, which represents the production of 50milliliters of CO2 in the reaction of HCl withNaHCO3. Five trials were performed under differentconditions as shown. (The same mass of NaHCO3 was used in each trial.)

A) trial A B) trial BC) trial C D) trial D

Which trial would produce the fastest reaction?

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A) It is exothermic and absorbs 286 kJ.B) It is endothermic and releases 286 kJ.C) It is exothermic and releases 286 kJ.D) It is endothermic and absorbs 286 kJ.

24. Given the reaction:

Which statement describes the reverse reaction?

A) 1 B) 2 C) 3 D) 4

25. Given the reaction:

N2(g) + 2 O2(g) 2 NO2(g)H = + 7.9 kcal/mole

The potential energy diagram of the reaction isshown below.

Which arrow represents the heat of reaction( H) for the reverse reaction?

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A) increasing B) constant C) decreasing D) zero

26. A reaction reaches equilibrium at 100 °C. The equation and graph representing this reaction areshown below.

The graph shows that the reaction is at equilibrium after 60 seconds because the concentration of bothNO2(g) and N2O4(g) are

A) concentrated B) diluteC) saturated D) unsaturated

27. A solution that is at equilibrium must be

A) less than the rate of liquid formationB) greater than the rate of liquid formationC) equal to the rate of liquid formation

28. A closed system is shown in the diagram below.

The rate of vapor formation at equilibrium is

A) the forward reaction, onlyB) the reverse reaction, onlyC) both the forward and reverse reactionsD) neither the forward nor reverse reaction

29. The addition of a catalyst to a system at equilibriumwill increase the rate of

A) decrease B) increaseC) remain the same

30. Given the reaction at equilibrium:

N2(g) + O2(g) « 2 NO(g)

As the concentration of N2(g) increases, theconcentration of O2(g) will

A) right and the concentration of Ag+ will increaseB) left and the concentration of Ag+(aq) will

increaseC) right and the concentration of Ag+ will decreaseD) left and the concentration of Ag+(aq) will

decrease

31. Given the system at equilibrium:

AgCl(s) « Ag+(aq) + Cl–(aq)

When 0.1 M HCl is added to the system, the point ofequilibrium will shift to the

A) Br2(s) at 266 K B) Br2( ) at 266 KC) Br2( ) at 332 K D) Br2(g) at 332 K

32. Which 1-mole sample has the least entropy?

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33. Base your answer to the following question on the information below.

At 550°C, 1.00 mole of CO2(g) and 1.00 mole of H2(g) are placed in a 1.00-liter reaction vessel. Thesubstances react to form CO(g) and H2O(g). Changes in the concentrations of the reactants and theconcentrations of the products are shown in the graph below.

What can be concluded from the graph about the concentrations of the reactants and theconcentrations of the products between time t 1 and time t 2?

34. Base your answer to the following question on the information below and on your knowledge ofchemistry.

Many breads are made by adding yeast to dough, causing the dough to rise. Yeast is a type ofmicroorganism that produces the catalyst zymase, which converts glucose, , to ethanoland carbon dioxide gas. The balanced equation for this reaction is shown below.

Describe how the catalyst, zymase, speeds up this reaction.

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Base your answers to questions 35 through 37 on the information below.

At room temperature, a reaction occurs when KIO3(aq) is mixed with NaHSO3(aq) that contains asmall amount of starch. The colorless reaction mixture turns dark blue after a period of time thatdepends on the concentration of the reactants.In a laboratory, 12 drops of a 0.02 M NaHSO3(aq) solution containing starch were placed in each ofsix test tubes. A different number of drops of 0.02 M KIO3(aq) and enough water to maintain aconstant volume were added to each test tube and the time for the dark-blue color to appear wasmeasured. The data were recorded in the table below.

35. Identify one factor, other than the concentration of the reactants, that would affect the rate of thisreaction.

36. State how increasing the number of drops of 0.02 M KIO3(aq) used in the reaction affects the rate ofreaction.

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37. On the grid below:Mark an appropriate scale on the axis labeled "Time (s)."Plot the data from the data table. Circle and connect the points.

Answer KeyKinetics and Equilibrium 2016

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1. B2. B3. C4. A5. A6. C7. A8. B9. A10. C11. C12. C13. B14. A15. A16. D17. C18. D19. A20. A21. D22. A23. D24. C25. B26. B27. C28. C29. C30. A31. D32. A

33. – Between time t 1 and time t 2, theconcentrations of thereactants and theconcentrations of theproducts are nolonger changing. –The concentrationsof the reactants andthe products remainconstant. – Theconcentration ofeach reactant is 0.73mol/L, and theconcentration ofeach product is 0.27mol/L.

34. — Zymase is acatalyst thatprovides analternative pathway,which requires lessenergy. — decreasesthe activation energy— changes thereaction mechanism

35. the temperature ofthe reactants or acatalyst

36. –Increasing thenumber of drops ofKIO3(aq) increasesthe rate of reaction.–The reaction takesless time if moredrops of KIO3 areused. –The reactionoccurs faster.

37.