Chemistry

The following reaction is first order, C2H6==> 2CH3. If the rate constant is equal to 5.5 x 10-4 s^-1 at 1000 K, how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.20 mol in the same container?

Thank you very much

  1. 👍 0
  2. 👎 0
  3. 👁 3,554
  1. ln(No/N) = kt
    ln(0.35/0.20) = kt
    Substitute for k and calculate t. The calculated time will be in seconds.

    1. 👍 0
    2. 👎 0
  2. ln(No/N) = kt
    ln(0.35/0.20) = kt
    ln(0.35/0.20)=1000*t
    ln(0.35/0.20)/(1000)=5.59

    but that answer is not on my worksheet im i doing something wrong?

    1. 👍 0
    2. 👎 0
  3. I'm not surprised. Why did you substitute 1000 for k? The problem states k = 5.5 x 10^-4 s^-1. You substituted 1000 Kelvin which is the temperature.

    1. 👍 1
    2. 👎 0
  4. oh haha i didn't notice i feel now

    1. 👍 0
    2. 👎 0
  5. ok i got i now thank you very much

    1. 👍 0
    2. 👎 0
  6. Chalk it up to "not focused" and work on focusing on the work at hand.

    1. 👍 0
    2. 👎 5
  7. i am trying to find tis answer but I m getting different result

    1. 👍 0
    2. 👎 0
  8. ln(No/N)
    =ln(0.35/0.20)
    = 0.559
    0.559/5.5*10-4
    =1017.48
    =17mins

    1. 👍 1
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. AP Chemistry

    C2H2(g) + 2H2(g) --> C2H6(g) Information about the substances involved in the reaction represented above is summarized in the following table: C2H2(g) 226.7 kj/mol C2H6(g) -84.7 kj/mol [the values are the change in enthalpy] a.

  2. 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

  3. chemistry

    The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 8.56× 10–10 cm3·molecule–1·s –1 at 298 K. convert to units of M-1 s-1. convert rate

  4. chemistry

    At constant pressure and 25 degrees C, what is delta H for the reaction 2C2H6(g) + 7O2(g) --yields-- 4CO2(g) + H2O(l) if the complete consumption of 11.3 g of C2H6 releases -586.3 kJ of heat energy? (11.3=.38 mol C2H6)

  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. Chemistry

    Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is: C2H2(g) + 2H2(g) === C2H6(g) Given the following, what is the Kp for the reaction? C2H2(g): 209.2 ΔG˚f (kJ/mol) H2(g): 0

  3. 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?

  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

    a first order reaction has a rate constant of 7.5 x 10^-3/s. The time required for th reaction to be 60% complete is

  2. General chemistry

    The first-order reaction, SO2Cl2---> SO2 + Cl2, has a rate constant equal to 2.20 x 10^-5 s^-1 at 593 K. What percentage of the initial amount SO2Cl2 will remain after 6.00 hours?

  3. Engineering Chemistry

    One reaction that destroys O3 molecules in the stratosphere is NO + O3 → NO2 + O2 When this reaction was studied in the laboratory, it was found to be first order with respect to both NO and O3, with a rate constant of 1.9 x 104

  4. chemistry help?!

    Which statement correctly pairs the order of a reaction with the units for the rate constant? A. third order; s/M B. zero order; 1/(M2) C. second order; 1/(M•s) D. first order; 1/M

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