Get 2 FREE Instant-Explanations on Filo with code FILOAPP

A first order reaction has k = 1.5 10^{-6} per second at 200^0

Question

A first order reaction has $k = 1.5 \times 1 0^{- 6}$ per second at $20 0^{0} C$ . If the reaction is allowed to run for 10 hrs, what percentage of the initial concentration would have changed into the product?

5.213%

10.21%

20.3%

15.2%

Views: 809 students

Found 3 tutors discussing this question

Amelia Discussed

A first order reaction has

k = 1.5 \times 1 0^{- 6}

per second at

20 0^{0} C

. If the reaction is allowed to run for 10 hrs, what percentage of the initial concentration would have changed into the product?

14 mins ago

Discuss this question LIVE

14 mins ago

Text solutionVerified

Given,

K = 1.5 \times 1 0^{- 6} s^{- 1}

We know for a first order reaction,

t = \frac{2.303}{K} l o g (\frac{N _{0}}{N})

So on substituting given values,

\frac{N _{0}}{N} = 1.0555

⟹ N = 0.9475 N_{0}

Now product formed

= 0.9475 N_{0} - N_{0} = 0.0521 N_{0} =

5.213%

Was this solution helpful?

151

Report

One destination to cover all your homework and assignment needs

Learn Practice Revision Succeed

Instant 1:1 help, 24x7

60, 000+ Expert tutors

Textbook solutions

Big idea maths, McGraw-Hill Education etc

Essay review

Get expert feedback on your essay

Schedule classes

High dosage tutoring from Dedicated 3 experts

Trusted by 4 million+ students

Stuck on the question or explanation?

Connect with our chemistry tutors online and get step by step solution of this question.

231 students are taking LIVE classes

Question Text	A first order reaction has $k = 1.5 \times 1 0^{- 6}$ per second at $20 0^{0} C$ . If the reaction is allowed to run for 10 hrs, what percentage of the initial concentration would have changed into the product?
Answer Type	Text solution:1
Upvotes	151