Rate constant and partial pressure

  • #1
brake4country
216
6

Homework Statement


The rate constant for the conversion of methyl isonitrile is 5 x 10^-5. A scientist has a container containing this substance with a partial pressure of 100 torr. After 12.8 hours (46,000 seconds), what is the partial pressure of methyl isonitrile gas inside the container?

Homework Equations


PV = nRT

The Attempt at a Solution


I tried to attempt this problem using concentrations but they were not given. I have no idea where to start...
 

Answers and Replies

  • #2
Borek
Mentor
29,100
3,710
Partial pressure is directly proportional to the concentration, so as long as there is no change in volume/total pressure they can be used interchangeably (simple conclusion of the Avogadro's law). But I have a different problem - I don't see how to solve, unless you are expected to assume first order reaction.
 
Last edited:
  • #3
epenguin
Homework Helper
Gold Member
3,931
962
Yes it sounds you are supposed to assume this. If we'd been told the units of the rate constant that would have told us. Bad! But if the OP knows what the question will have that answered.

We're not even told what the reaction is. Again from the absence of information we'd guess probably just rearrangement to acetonitrile. Again quite plausibly but not necessarily that is just a monomolecular internal movement that could be first order.
 
  • #4
brake4country
216
6
Yes, I just realized that the book has this equation: log [A]t=-kt/2.303 + log[A]0 for a first order reaction. So this is a first order reaction. This looks like plug and chug:

log[A]t = -(5x10-5)(46000)/2.303) + log [100]
log[A] = -1+2 = log[A} = 1 therefore, the answer is 10 torr.

My other question is that I had to use a calculator for this problem but the test does not allow calculators. How best to approach this type of problem without a calculator? Thanks in advance!
 
  • #5
epenguin
Homework Helper
Gold Member
3,931
962
Yes, I just realized that the book has this equation: log [A]t=-kt/2.303 + log[A]0 for a first order reaction. So this is a first order reaction. This looks like plug and chug:

log[A]t = -(5x10-5)(46000)/2.303) + log [100]
log[A] = -1+2 = log[A} = 1 therefore, the answer is 10 torr.

My other question is that I had to use a calculator for this problem but the test does not allow calculators. How best to approach this type of problem without a calculator? Thanks in advance!

In general you can't. It would not be reasonable to ask you do so and it will not happen - unless the problem had nice round numbers like this one. It was reasonable to expect you to know the log of 100 and the antilog of 1.

You would find it kinda useful often if you mastered an art of mentally converting 1st order rate constants to half-lives.

So would I. :biggrin:
 

Suggested for: Rate constant and partial pressure

Replies
2
Views
536
Replies
4
Views
542
  • Last Post
Replies
16
Views
1K
  • Last Post
Replies
1
Views
640
  • Last Post
Replies
16
Views
1K
Replies
2
Views
436
Replies
12
Views
2K
  • Last Post
Replies
1
Views
521
Replies
3
Views
1K
  • Last Post
Replies
5
Views
492
Top