Question

# H2O2 decomposes at 20˚C in a first order reaction where k = 1.06 x 10-3min-1. If...

H2O2 decomposes at 20˚C in a first order reaction where k = 1.06 x 10-3min-1. If the initial concentration of H2O2 is 0.020 M, what is [H2O2] after 3.5 days?

 a. 9.6x10-5 M b. 5.1x10-5 M c. 4.4x10-5 M d. 1.7x10-5 M

For the following reaction, calculate the average reaction rate over the last 2 minutes using the table of data below.

H2(g)   +   2ICl(g)      I2(g)   +   2HCl(g)

Time (min)     [ICl] (M)

--------------     -----------

0             2.000

2                1.052

4                0.748

6                0.586

 a. 0.0900 M/min b. 0.175 M/min c. 0.0405 M/min d. 0.352 M/min
1. Which statement(s) below do we know is (are) true about the following net reaction?

2N2O5      2N2   +   5O2

 a. The rate law = k[N2O5]2 b. The reaction rate = 1/2(∆[N2]/∆t) c. The reaction rate = 1/2(∆[N2O5]/∆t) d. The reaction rate = -1/5(∆[O2]/∆t) e. a & b f. b & c g. c & d h. a, b, & c i. b, c, & d j. All are true

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