If the rate of decomposition of potassium chlorate at a certain time is determined to be 2.4 x 10-2 mol s-1. What is the rate of formation of O2 at the same time?
1.6 x 10-2 mol s-1
2.4 x 10-2 mol s-1
3.6 x 10-2 mol s-1
1.2 x 10-2 mol s-1
7.2 x 10-2 mol s-1
For a second order reaction with a rate constant k = 3.13 x 102 L mol-1 s-1, how long does it take for the concentration of the only reactant to become 70% of the original amount?
0.0761 seconds
0.00137 seconds
0.00746 seconds
0.912 seconds
0.00114 seconds
For the following reaction:
A → B + C
that is second order, a linear plot will result when time is plotted against:
ln[B]
ln[B][C]
[A]
1/[A]
ln[A]
For a first order reaction with a rate constant k = 3.13 x 102 s-1, how long does it take for the concentration of the only reactant to become 40% of the original amount?
0.00128 seconds
0.00479 seconds
0.00293 seconds
43.2 seconds
0.0450 seconds
Catalysts lower the activation energy of a reaction by:
adding heat to the reaction system
increasing the energy content of the reactants
providing an alternate pathway for the reaction
none of these
changing the value of DH for the reaction
For a reaction between X and Y, the following data was obtained:
[X]0
[Y]0
Initial Rate
0.10
0.10
2.0 x 103
0.20
0.10
4.0 x 103
0.10
0.20
8.0 x 103
What is the rate law for this reaction?
R = k[X]2[Y]
R = k[Y]2
R = k[X][Y]
R = k[X][Y]2
R = k[X]2[Y]2
The following data give the concentration of gaseous butadiene as a function of time at 500 K. Determine the order of the reaction, and the value of the rate constant.
t(sec)
C(moles/liter)
195
1.62 x 10-2
604
1.47 x 10-2
1246
1.29 x 10-2
2180
1.10 x 10-2
4140
0.89 x 10-2
4655
0.80 x 10-2
6210
0.68 x 10-2
8135
0.57 x 10-2
first order, k = 1.4 x 102 s-1
second order, k = 1.4 x 102 L mol-1s-1
zero order, k = -1.4 x 10-2 mol L-1s-1
first order, k = 1.4 x 10-2 L mol-1s-1
second order, k = 1.4 x 10-2 L mol-1s-1
Increasing the temperature at which a reaction occurs speeds up the reaction by:
activating catalysts
increasing the energy of collisions
improving the orientation of collisions
two of these
increasing the frequency of collisions
For a first order reaction with a rate constant k = 1.2 x 10-3s-1, how long will it take for the amount of reactant to be decreased from 0.10 mol to 0.05 mol?
none of these
6.7 seconds
8.3 x 102 seconds
8.3 x 103 seconds
580 seconds
Which of the following statements is TRUE for the catalyzed and uncatalyzed versions of the same reaction?
DE is the same
The activation energies are the same
The energy content of the activated complex is higher for the catalyzed reaction
The energy content of the reactants is higher for the uncatalyzed reaction
The reaction pathway is the same
The reaction X2Y → 2X + Y is determined to be first order. What is the integrated rate law for this reaction?
(1/[X2Y]) = -kt + (1/[X2Y]0)
[X2Y] = -kt + [X2Y]0
ln[X2Y] = -kt + ln[X2Y]0
(1/[2X + Y]) = -kt + (1/[2X + Y]0)
ln[2X + Y] = kt - ln[2X + Y]0
A certain first-order reaction is 50.0% complete in 4.25 minutes. What is the rate constant for this reaction?
2.95 min
6.13 min
0.163 min-1
0.0252 min-1
[A]0/(2t1/2)
The rate law for a particular reaction is determined to be R = k[A]2[B]2. What is the overall order for this reaction?
third
fourth
second
first
zero
A certain first order decomposition reaction reaches 65% completion in 18.9 seconds. What is the rate constant for this reaction?
2.38 x 10-2 s-1
19.8 s-1
18 s-1
9.56 x 10-2 s-1
5.55 x 10-2 s-1
The activation energy for the reaction:
X2(g) + Y2(g) → 2XY(g)
is 125 kJ/mol and DE for the reaction is -45 kJ/mol. The activation energy for the decomposition of XY is: