Chemistry

The following rearrangement reaction is first order:

C3H6 �¨ CH3CH=CH2

The rate constant for this reaction is 6.7 �~ 10−4. How many minutes will it take for the concentration of C3H6 to drop to 11.75% of its initial value?

How do I calculate this step by step.
My answer was 3.1 minutes and it was wrong.

  1. 👍 0
  2. 👎 0
  3. 👁 231
  1. You don't have any units on k. Also, I'm not sure I've translated the mumbo jumbo symbols you have correctly so check the below carefully.

    ln(No/N) = kt
    No = 100
    N = 11.75
    k = 6.7E-4 (min^-1 or sec^-1 or whatever)
    t = time and the time will be minutes, seconds, hours, days, or whatever the unit of k. Then time will need to be convert to minutes if k is in some unit other than minutes.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    At a given temperature, a first-order reaction has a rate constant of 3.5 ´ 10–3 s–1. How long will it take for the reaction to be 24% complete? A chemical reaction that is first-order in X is observed to have a rate constant

  2. Kinetics Problem II

    The data below were collected for the following reaction: 2NO2 (g) + F2 (g) ->2NO2F(g) A: Calculate the value of the rate constant, k. B: What is the overall order of the reaction?

  3. CHEM- KINETICS

    The rate constant for a reaction is 4.65 L mol-1s-1. The overall order of the reaction is: zero first second third I am having trouble with the order of reactions. I don't understand this question. this is an assignment question

  4. Chemistry

    The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) „_ 2 NO2(g) The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.7 x 10^2

  1. Chemistry

    For the reaction 2 NO (g) + Cl2 (g) → 2 NOCl (g) If the concentration of NO is tripled, the rate of the reaction increases by a factor of nine. If the concentration of Cl2 is cut in half, the rate of the reaction is decreased to

  2. Chemistry

    The rate constant for a second-order reaction is 0.54 M-1s-1. What is the half-life of this reaction if the initial concentration is 0.27 M

  3. chemistry

    1. All of the following are structural isomers of CH2=CHCH2CH=CHCH3 EXCEPT a. CH2=CHCH2CH2CH=CH2 b. CH3CH=CHCH2CH=CH2 c. CH3CH=CHCH=CHCH3 d. CH2=C=CHCH2CH2CH3 Is it D? 2. Almost all of the amoino acids found in living organisms

  4. Chemistry

    A student tested the effect of temperature on the decomposition of N2O5. He found that the rate of the reaction at a lower temperature was 4.2 x 10–3 s–1 and the rate at a higher temperature was 1.6 x 101 s–1. What is wrong

  1. Chemistry

    What change do you expect if the value of the reaction quotient is greater than the value of the equilibrium constant? A- Rate of the forward reaction is greater than the rate of the reaction B- The rate of the forward reaction is

  2. chemistry

    A student performed two side-by-side reactions to test the decomposition of N2O5. The only difference between the two reactions was reactant concentration — reaction 1 started with 2 M N2O5 and reaction 2 started with 1.2 M.

  3. Chemistry

    A reaction is first order in A. If the rate constant of the reaction is 3.45x10^-3 s-1, what is the half life of the reaction? a. 4.98x10^-3 s b. 200 s c. 3.45x10^-3 s d. 100 s e. 1.73x10^-3 s

  4. Chemistry

    Study the chemical reaction. A + B ⟶ C + D A scientist studying this reaction states the reaction is first order with regard to A and zeroth order with regard to B. What is the rate law for this reaction? Rate = K [A] Rate = K

You can view more similar questions or ask a new question.