Question

Question #5 Here are the relevant data to determine the activation energy of the reaction. Rate constant (units not shown) Te
You have determined the numerical values of the rate constants for the catalyzed reaction (13) and the uncatalyzed reaction (
0 0
Add a comment Improve this question Transcribed image text
Answer #1

vant Hoff equation, en la ) OH (-+) en C4) - Saint Laurentre) 8.314x 0. 1670 = 1 1 1 3 - 1 308) Ea 308 Ea- 8853.214 I/mol Ea

Add a comment
Know the answer?
Add Answer to:
Question #5 Here are the relevant data to determine the activation energy of the reaction. Rate...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • question 5,6 part 1 and 2 please Question #5 Here are the relevant data to determine the activation energy of the...

    question 5,6 part 1 and 2 please Question #5 Here are the relevant data to determine the activation energy of the reaction. Rate constant (units not shown) Temperature (K) .13 293 0.11 308 Use the data above to determine the activation energy of the reaction. -3628 kl/mol Submit Please enter your results to the correct precision. Question #6 Here are your data for trial of Lab 7 (the trial at room temperature without the catalyst): [103 initial (S2032 Jinitial Initial...

  • The activation energy of a certain uncatalyzed biochemical reaction is 46.7 kJ/mol. In the presence of...

    The activation energy of a certain uncatalyzed biochemical reaction is 46.7 kJ/mol. In the presence of a catalyst at 39ºC, the rate constant for the reaction increases by a factor of 2030 as compared with the uncatalyzed reaction. Assuming the frequency factor A is the same for both the catalyzed and uncatalyzed reactions, calculate the activation energy for the catalyzed reaction. Activation energy =  kJ/mol

  • A catalyst lowers the activation energy for a particular reaction from 75.0 kJ mol−1to 40.0 kJ...

    A catalyst lowers the activation energy for a particular reaction from 75.0 kJ mol−1to 40.0 kJ mol−1. By what factor does the rate constant increase if the catalyst is used at 25.0 °C? Assume that all rate constants obey the Arrhenius equation and that the pre-exponential factors for the uncatalyzed and catalyzed reactions are equal

  • 1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for...

    1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for the reaction increases from 93.5 M-1s-1 at 497.7 K to 1349.3 M-1s-1 at 636.7 K. do not include units, but make sure your answer is in kJ/mol! 2) A chemist constructs a plot of ln k vs. 1/T for a chemical reaction. The slope of the trendline for the data is -746 K. What is the activation energy for this reaction in kJ/mol? R...

  • The activation energy for a reaction is changed from 184 kJ/mol to 58.1 kJ/mol at 600....

    The activation energy for a reaction is changed from 184 kJ/mol to 58.1 kJ/mol at 600. K by the introduction of a catalyst. If the uncatalyzed reaction takes about 2574 years to occur, about how long will the catalyzed reaction take? Assume the frequency factor A is constant and assume the initial concentrations are the same.

  • Using the Arrhenius equation to calculate the activation energy. The rate constant of a chemical reaction...

    Using the Arrhenius equation to calculate the activation energy. The rate constant of a chemical reaction increased from 0.100s-1 to 2.90s-1 upon raising the temperature from 25 to 45 C (1/t2 -1/t1)= -2.11x10^-4 K-1 Calculate the value of In (k1/k2) where k1 and k2 corresponds to the rate constant at the initial and the final temperature as found above. In(k1/k2)=?? Also, what is the activation energy of the reaction? Expressed in kilojoules per mile Ea=??

  • Use the Arrhenius equation to calculate the activation energy. The rate constant of a chemical reaction...

    Use the Arrhenius equation to calculate the activation energy. The rate constant of a chemical reaction increased from 0.100 s−1 to 2.70 s−1 upon raising the temperature from 25.0 ∘C to 43.0 ∘C . a) Calculate the value of (1/T2−1/T1) where T1 is the initial temperature and T2 is the final temperature. (in units of k-1) b) Calculate the value of ln(k1/k2) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined...

  • 3,4,5!!! please Question #2 Here are your data for trials 1-4 of Lab 7: [103 initial...

    3,4,5!!! please Question #2 Here are your data for trials 1-4 of Lab 7: [103 initial (S203 Jinitial Initial rate Trial 1 .0023 M 1 .00090 M .000028 M/s Trial 2 .0047 M .00090 M .000069 M/S Trial 3 .0023 M .0018 M .000052 M/S Trial 4 .0047 M .0018 M .000058 M/s The order with respect to 10, should be an integer (either 0, 1, or 2). Let's determine it using two sets of data: Part 1: Use the...

  • INFORMATION reaction must also be perimental mea data are plotted in the sult means that the...

    INFORMATION reaction must also be perimental mea data are plotted in the sult means that the rate Because a reaction is faster at higher temperatures, the rate constant for the reaction m larger. The activation energy of a reaction can therefore be determined from experime surements of the rate constant at several temperatures. When the collected data are ple form In(k) vs T. as shown in Figure 2. a straight line is produced. This result means constant varies exponentially with...

  • To use the Arrhenius equation to calculate the activation energy. As temperature rises, the average kinetic...

    To use the Arrhenius equation to calculate the activation energy. As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation k=Ae−Ea/RT where k is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.3145 J/(K⋅mol) is the gas constant, and T is the...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT