Rate order I hardly know her
What is the overall order of the reaction
Rate = k[A]2[B]
Third order
A catalyst speeds up a reaction by ___ the activation energy
lowering
A reaction has the stoichiometry: 2A+B→3C
If C is being produced at 0.60 M/s, at what rate is A being consumed?
0.4 M/s
What are the units for k for a zero-order reaction?
M/s
What does the A constant in the Arrhenius equation stand for?
frequency factor
For a reaction, the concentration of A is doubled while all other concentrations remain constant. The reaction rate increases by a factor of 4.
What is the reaction order with respect to A?
2nd order
As the temperature increases, the number of collisions per second will ______
increase
For the reaction: A+2B→C
the concentration of B decreases from 0.80 M to 0.50 M in 15.0 s.
What is the average rate of reaction?
0.01 M/s
A reaction follows:
R=k[A][B]2
When [A]=0.20 M and [B]=0.50 M, the reaction rate is 0.010 M/s
What is the value of k?
0.20 M-2s-1
Rate=k[A]2[B]
The concentration of A is tripled, while the concentration of B is cut in half.
By what factor does the reaction rate change?
4.5
The concentration of a reactant declines linearly with time as a reaction proceeds.
What is the rate order?
Zeroth order
A species that is made in the first step and used in the second step is called what?
intermediate
True or False: "If the concentration of a reactant decreases by 0.20 M over 10 seconds, the reaction rate must be 0.020 M/s."
False
What is the slope on a graph of 1/[A] vs. time for a second order process?
+k
A first order decay process is 30% complete in 7.0 min. At what time would the reaction be 87% complete?
40 minutes
A graph of rate vs concentration shows a straight line increasing. What rate order is it?
1st order
A species that is used in the first step and regenerated in the second step is called what?
catalyst
For the reaction:
2NO+O2→2NO2
a student measures the rate of disappearance of NO and obtains: −Δ[NO]/ Δt = 0.080 M/s
Which statement is TRUE?
A) The reaction rate is 0.080 M/s.
B) O2 is consumed at 0.080 M/s.
C) NO2 is produced at 0.040 M/s.
D) NO2 is produced at 0.080 M/s.
E) O2 is consumed at 0.020 M/s.
D) NO2 is produced at 0.080 M/s.
What are the units of k for a reaction with a Rate = k[A]2[B]?
M-2s-1
A chemical decays by a second-order process. When the initial concentration is 0.57 M, t1/2 = 13 sec. At what time will the concentration of this chemical be 0.30 M?
11.7 seconds
A reaction follows the rate law
Rate = k[A]2[B]
If the concentration of A is cut in half while the concentration of B is tripled, by what factor does the reaction rate change?
Rate decreases by a factor of 4/3
The rate constant for a first-order reaction was 3.19 x10-7 sec-1 at 245 C and 5.67 x 10-6 sec-1 at 413 C.
What is the energy of activation in kJ?
50.6 kj/mol
For the reaction: 2A+3B→4C
the concentration of A changes from 0.800 M to 0.500 M in 15.0 s.
What is the average rate of formation of C during this time?
0.04 M/s
A reaction obeys: Rate = k[A]2[B]
At one instant, [A]=0.250 M, [B]=0.400 M[B]=0.400, and the reaction rate is 0.0500 M/s
What is the rate when [A] decreases to 0.100 M while [B] remains 0.400 M?
0.008 M/s
A proposed mechanism for the stoichiometric reaction:
A + B → C
involves two steps…
Step 1: A + B → I fast
Step 2: I → C slow
If the mechanism were correct, what should be the overall rate-law expression?
Rate = k[A][B]