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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