• #### 1.  What is the rate law for this mechanism?

• rate = k[A][B]2
• rate = [B][X]
• rate = [A]0.5[B]1.5
• rate = [W][Y][Z]

• Diffusion
• Big Bang
• Collusion
• Evalusion

• .01704 M/s
• .0852 M/s
• .1704 M/s
• .852 M/s
• #### 4.  A possible rate law for a third overall order of a reaction is __________________

• Rate = k [A]2[B]2
• Rate = k [A][B]3
• Rate = k [A]3 [B]
• Rate = k [A]2[B]

• zero
• one
• two
• three
• #### 6.  The time in which half of the substance has reacted is

• Half life period
• Full life time
• Both 1,2
• None of the above

• A
• B
• C
• D
• #### 8.  Consider the following rate law: Rate = k[A]n[B]mHow are the exponents n and m determined?

• by using balanced chemical equation
• By using the subscripts for the formulas
• By educated guess
• By experiment
• #### 9.  Given the following rate law, rate = k[A]2[B]if [A] were doubled, what must happen to [B] to keep the rate constant?

• [B] must double
• [B] must be havled
• [B] must be quartered
• #### 10.  Which of the following is NOT a factor affecting reaction rate?

• temperature
• catalysts
• particle size
• polarity

• 50 mins
• 30 mins
• 40 mins
• 60 mins
• #### 12.  The following data were measured for the reaction BF3(g) + NH3(g) ⟶ F3BNH3(g)What is the rate law for the reaction?

• rate = k[NH3]
• rate = k[BF3]2[NH3]
• rate = k[BF3][NH3]
• rate = k[BF3][NH3]2
• #### 13.  Decreasing the particle size increases the reaction rate because

• It makes particles move faster
• It increases the likelihood of collisions with the correct geometry
• It decreases the surface area available to react
• It increases the number of collisions

• 1.26×1015 s
• 2.52×1014 s
• 2.52×1028 s
• infinite

• k = AeEa/RT
• k = Ae-Ea/RT
• k = AeRT/Ea
• k = Ae-RT/Ea
• #### 16.  Reaction rate means...

• amount of product formed
• speed of reaction
• concentration of reacting particles
• combining reactants with products
• #### 17.  Which of the following best describes why increasing temperature increase reaction rate?

• Activation energy is reduced.
• Collisions become more frequent.
• Collisions become more energetic.
• Collisions become more frequent and more energetic.
• #### 18.  Rate = k[A]The rate constant in the rate law above is 0.5 L/mol·s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

• 0.7 s
• 1.4 s
• 2.8 s
• There is not enough information given.
• #### 19.  The catalyst alters the rate of a chemical reaction by,

• providing an alternative pathway with a lower Ea
• changing the products formed in the direction of the reaction
• providing a surface on which the molecules react
• increasing the frequencies of collisions between molecules

• M/s
• mol/s
• m.s
• s/M
• #### 21.  Given the following balanced equation : 2NO(g) + Cl2(g) → 2NOCl(g)If the rate of disappearance of Cl2 is 4.84 x 10-2 Ms-1, what is the rate of disappearance of NO?

• 1.45 x 10-2 Ms-1
• 2.42 x 10-2 Ms-1
• 3.67 x 10-2 Ms-1
• 9.68 x 10-2 Ms-1

• 1
• 1.5
• 2
• 2.5

• Potential
• Kinetic
• Activation
• Conversion

• I
• II
• III
• I and II
• #### 25.  Which species is the catalyst in this reaction mechanism?

• R
• W
• X
• There is no catalyst.
• #### 26.  The iodide ion reacts with hypochlorite ion in the following way:OCl- + I- ⟶ OI- + Cl-.This rapid reaction gives the rate data shown. What is the rate law?

• rate = [OCl-]2[I-]
• rate = [OCl-][I-]2
• rate = [OCl-][I-]
• rate = [OCl-]

• second order
• first order
• zero order
• third order
Report Question
access_time