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

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
For the first order decomposition of H2O2(aq), given k = 3.60 x 10-3 s-1 and the...
For the first order decomposition of H2O2(aq), given k = 3.60 x 10-3 s-1 and the initial concentration of [H2O2]o is 0.882 M, determine : (a) the time at which [H2O2]t decreases to 0.600 M; (b) what will be the concentration of [H2O2]t after 225 s and (c) find the half-life of the reaction.
The first order constant is 4.82 x 10-3 s-1 at 70C for the decomposition of the...
The first order constant is 4.82 x 10-3 s-1 at 70C for the decomposition of the following reaction: 2N2O5 (g) -> 4NO2 + O2 (g) Suppose that you start with .0175M of N2O5 (g) a.) What is the molarity of N2O5 that remains after 15 minutes (note: the rate constant is in seconds) b.) How many seconds will it take for the quantity of N2O5 to drop to .015M? c.) What is the half life of N2O5 at 70C?
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)?4NO2(g)+O2(g), at 70?C is 6.82×10?3s?1. Suppose we...
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)?4NO2(g)+O2(g), at 70?C is 6.82×10?3s?1. Suppose we start with 2.90×10?2 mol of N2O5(g) in a volume of 1.5 L . a) How many moles of N2O5 will remain after 5.0 min ? b) How many minutes will it take for the quantity of N2O5 to drop to 2.0×10?2 mol? c) What is the half-life of N2O5 at 70?C?
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose...
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose we start with 2.30×10−2 mol of N2O5(g) in a volume of 1.8 L . a) How many moles of N2O5 will remain after 6.0 min ? b) How many minutes will it take for the quantity of N2O5 to drop to 1.6×10−2 mol ? c) What is the half-life of N2O5 at 70∘C?
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10^−3 s−1. Suppose...
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10^−3 s−1. Suppose we start with 2.60×10^−2 mol of N2O5(g) in a volume of 2.4 L . How many moles of N2O5 will remain after 4.0 min ? How many minutes will it take for the quantity of N2O5 to drop to 1.9×10^−2 mol ? What is the half-life of N2O5 at 70∘C?
The rate constant for the first-order decomposition of N2O5 by the reaction 2 N2O5 (g) ...
The rate constant for the first-order decomposition of N2O5 by the reaction 2 N2O5 (g)  4 NO2(g) + O2(g) is k, = 3.38 x 10-5 s -1 at 25 C. What is the half-life of N2O5? What will be the partial pressure, initially 500 Torr, at ( a) 50 s; (b) 20 min, (c) 2 hr after initiation of the reaction?
The decomposition of hydrogen peroxide (H2O2) is a first order reaction with a rate constant 1.8×10-5...
The decomposition of hydrogen peroxide (H2O2) is a first order reaction with a rate constant 1.8×10-5 s -1 at 20°C. (a) What is the half life (in hours) for the reaction at 20°C? (b) What is the molarity of H2O2 after four half lives if the initial concentration is 0.30 M? (c) How many hours will it take for the concentration to drop to 25% of its initial value? *Help please!!!*
1) The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½...
1) The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3 min-1. If the initial concentration of H2O2 is 9.20×10-2 M, the concentration of H2O2 will be 1.83×10-2 M after____________ min have passed. 2) The gas phase decomposition of dimethyl ether at 500 °C CH3OCH3(g) CH4(g) + H2(g) + CO(g) is first order in CH3OCH3 with a rate constant of 4.00×10-4 s-1. If...
1. Dinitrogen pentoxide (N2O5) decomposes to NO2 and O2 at relatively low temperatures in the reaction...
1. Dinitrogen pentoxide (N2O5) decomposes to NO2 and O2 at relatively low temperatures in the reaction 2N2O5(soln) → 4NO2(soln) + O2(g) This reaction is carried out in a CCl4 solution at 45° C. The concentrations of N2O5 as a function of time are listed in the table. Plot a graph of the concentration versus t, ln (natural log) concentration versus t, and 1/concentration versus t. Graphically, determine the order of the reaction, write the rate law and calculate the value...
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose...
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose we start with 2.10×10−2 mol of N2O5(g) in a volume of 1.8 L . How many minutes will it take for the quantity of N2O5 to drop to 1.6×10−2 mol ?