# Kinetics

## Quiz by Natalie Wieland

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13 questions
• Q1
The rate law of a reaction is determined to be rate = k[A][B]2. Which statement would most likely describe the reaction?
The stoichiometry of the overall reaction must be A+2B--> products
The reaction involves a one-step, termolecular mechanism
The reaction involves the formation of intermediates
The reaction is catalyzed by an enzyme
60s
• Q2
In the reaction NO3(g) + CO(g) <=> NOw(g) + CO2(g), the carbon in CO must collide with an oxygen in NO3 with sufficient energy to react. Which of the diagrams below would most likely result in the formation of products?
60 C and right orientation
80 C and wrong orienation
100 C somewhat right orientation
-40 C and right orientation
60s
• Q3
The graph above shows the number of molecules that have sufficient energy to overcome Ea for a given reaction. How would adding an enzyme change the appearance of the graph?
no change in the graph
lowers the height of the graph
same shape but the activation energy has been lowered
shifts the graph further to the right
60s
• Q4
The values for the change in enthalpy, dH, and the activation energy, Ea, for a given reaction are known. The value of Ea for the reverse reaction equals
the sum of dH and Ea
the sum of -dH and Ea
-(Ea) for the forward reaction
Ea for the forward reaction
60s
• Q5
For two first-order reactions of different substances A and X, A-->B t1/2 = 30.0 min, X-->Y t1/2 = 60.0 min. This means that
the rate constant for A-->B is lower than the rate constant of X-->Y
3 moles of A will react more rapidly than 3 moles of X
a certain number of grams of A will react twice as fast as the same number of grams of X
a certain number of grams of X will react twice as fast as the same number of grams of A
60s
• Q6
A reaction is first order with respect to [X] and second order with respect to [Y]. When [X] is 0.20M and [Y]=0.20M the rate is 8.00x10-3Mmin-1. The value of the rate constant, including correct units, is
2.0 M-2min-1
1.00 Mmin-1
2.00 M-1min-1
1.00 M-2min-1
60s
• Q7
The activation energy for this reaction, X+2Y-->3Z, shown in the potential energy diagram, could be
increased by increasing [X] and [Y]
decreased by adding a suitable catalyst
decreased by removing Z from the system as it forms
increased by increasing the temperature
60s
• Q8
For all zero-order reactions
the rate is independent of time
Ea is very low
a plot of time vs. concentration squared is linear
the concentration of reactants is constant
60s
• Q9
Use the following information. Carbon monoxide reacts with oxygen according to the equation CO(g) + 1/2O2(g) --> CO2(g). The rate law for the reaction is: Rate = k[CO]m[O2]n. Experimental information for the reaction is given in the following table. Which values correspond to the reaction orders m and n for CO and O2?
m = 2, n = 1
m = 1, n = 1/2
m = 1, n = 1
m = 4, n = 2
60s
• Q10
What is the overall reaction order?
2
1
0
3
60s
• Q11
What is the numerical value of the rate constant, k, for this reaction?
1.54x10 4 min-1
3.68x10-5 molL-1min-1
2.93x10-25 molmin-1
4.60 L2mol-2min-1
60s
• Q12
Which of the following statements would be correct regarding the following reaction? 2H2(g) + Ox(g) --> 2H2O(g)
The rate of H2O disappearance is equal to the rate of O2 disappearance
The rate of H2 disappearance is twice the rate of O2 disappearance
The rate of H2O disappearance is twice the rate of O2 disappearance
The rate of O2 disappearance is twice the rate of H2 disappearance
60s
• Q13
According to the collision theory of kinetics, which statement best describes the rate of a chemical reaction?
The greater the difference in energy between the reactants and the products, the faster is the raction
All collisions result in a chemical reaction
All collisions between molecules with at least a minimum kinetic energy and the proper orientation result in reaction
All collisions between molecules with at least a minimum kinetic energy result in reaction
60s

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