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Q 1/13
Score 0
The rate law of a reaction is determined to be rate = k[A][B]2. Which statement would most likely describe the reaction?
60
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
Q 2/13
Score 0
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
60 C and right orientation
80 C and wrong orienation
100 C somewhat right orientation
-40 C and right orientation
13 questions
Q.
The rate law of a reaction is determined to be rate = k[A][B]2. Which statement would most likely describe the reaction?
1
60 sec
Q.
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?
2
60 sec
Q.
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?
3
60 sec
Q.
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
4
60 sec
Q.
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
5
60 sec
Q.
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
6
60 sec
Q.
The activation energy for this reaction, X+2Y-->3Z, shown in the potential energy diagram, could be
7
60 sec
Q.
For all zero-order reactions
8
60 sec
Q.
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?
9
60 sec
Q.
What is the overall reaction order?
10
60 sec
Q.
What is the numerical value of the rate constant, k, for this reaction?
11
60 sec
Q.
Which of the following statements would be correct regarding the following reaction? 2H2(g) + Ox(g) --> 2H2O(g)
12
60 sec
Q.
According to the collision theory of kinetics, which statement best describes the rate of a chemical reaction?
