HomeworkLib
Question

The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42X10^-4 at a...

What is the half life?



How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration?





If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.74 M?




PLEASE EXPLAIN WHY YOU DO EACH OF THESE STEPS SO I CAN DO THIS ON A QUIZ.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Request Professional Answer

Request Answer!

We need at least 10 more requests to produce the answer.

0 / 10 have requested this problem solution

The more requests, the faster the answer.

Request! (Login Required)

All students who have requested the answer will be notified once they are available.
Know the answer?
Add Answer to:
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42X10^-4 at a...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Similar Homework Help Questions

  • The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10−4...

    The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10−4 s−1 at a certain temperature. A) How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration? Express your answer using two significant figures. B)If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.74 M ? Express your answer using two significant figures. Please explain step...

  • The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42...

    The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42 * 10 - 4 s - 1 at a certain temperature. a. What is the half-life for this reaction? b. How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration? c. If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.78 M? d. If the...

  • The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.48×10−4...

    The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.48×10−4 s−1 at a certain temperature. How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration? If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.76 M ? If the initial concentration of SO2Cl2 is 0.175 M , what is the concentration of SO2Cl2 after 210...

  • The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.40×10−4...

    The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.40×10−4 s−1 at a certain temperature. Part A Part complete What is the half-life for this reaction? t1/2 = 4950   s   SubmitPrevious Answers Correct Part B Part complete How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration? Express your answer using two significant figures. t = 9900   s   SubmitPrevious Answers Correct Part C Part complete If...

  • The decomposition of SO2Cl2 is first order in SO, Cl, and has a rate constant of...

    The decomposition of SO2Cl2 is first order in SO, Cl, and has a rate constant of 1.38x10-4 5-1 at a certain temperature. Part A What is the half-life for this reaction? ΟΙ ΑΣφ ? 11/2= Submit Request Answer Part B How long will it take for the concentration of SO, Cl, to decrease to 25% of its initial concentration? Express your answer using two significant figures. ΟΙ ΑΣΦ ? Part C If the initial concentration of SO, Cl, is 1.00...

  • The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.36×10−4...

    The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.36×10−4 s−1 at a certain temperature. Part A: If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.78 M ? Part B: If the initial concentration of SO2Cl2 is 0.125 M , what is the concentration of SO2Cl2 after 180 s? Part C: If the initial concentration of SO2Cl2 is 0.125 M , what...

  • The first order reaction, SO2Cl2 --> SO2 + Cl2, has a half life of 8.75 hours...

    The first order reaction, SO2Cl2 --> SO2 + Cl2, has a half life of 8.75 hours at 593 K.? How long will it take for the concentration of SO2CL2 to fall to 12.5% of its initial value? Steps must be shown.

  • The decomposition of SO,Cl, is first order in SO, Cl, and has a rate constant of...

    The decomposition of SO,Cl, is first order in SO, Cl, and has a rate constant of 1.38x10 - at a certain temperature Part A What is the half-life for this reaction? 1 | ΑΣφ και ? $ Submit Het we Part How long wil it take for the concentration of SO,Cl to decrease to 25% of its initial concentration? Express your answer using two significant figures. VE ΑΣφ ? Submit Beavest A The decomposition of SO,Cl is first order in...

  • 4) If the reaction SO2Cl2 → SO2 + Cl2 is first-order reaction. At 230oC, k =...

    4) If the reaction SO2Cl2 → SO2 + Cl2 is first-order reaction. At 230oC, k = 0.125 hr-1. If the initial concentration of SO2Cl2 is 0.250 M, what is the concentration after 7.6 hours? How long will it take for the concentration of SO2Cl2 to drop to 0.0651 M? What is the half-life for this first order reaction?

  • The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42*10^-4...

    The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42*10^-4 1/s at a certain temperature. How long will it take for the reaction to be 75.0% complete?

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