Question

Part A A certain first-order reaction has a rate constant of 3.00×10−2 s−1 at 25 ∘C...

Part A

A certain first-order reaction has a rate constant of 3.00×10−2 s−1 at 25 ∘C . What is the value of k at 69 ∘C if Ea = 77.0 kJ/mol ?

Express your answer using two significant figures.

Part B

Another first-order reaction also has a rate constant of 3.00×10−2 s−1 at 25 ∘C . What is the value of k at 69 ∘C if Ea = 115 kJ/mol ?

Express your answer using two significant figures.

Homework Answers

Answer #1

Part A)

We know the formula

ln(k2/k1)=(-Ea/RT2)+(Ea/RT1)

So by putting given values in above formula , we get

ln(k2/ 3.00 x 10−2 s−1 ) = (-77000 J/mol / (8.31 x 342 K ) + ( 77000 J/mol / (8.31 x 298 K )

ln(k2/ 3.00 x 10−2 s−1 ) =   4.00

So

k2 = e4 x 3.00 x 10−2 s−1

= 1.63 s−1

Part B)

We know the formula

ln(k2/k1)=(-Ea/RT2)+(Ea/RT1)

So by putting given values in above formula , we get

ln(k2/ 3.00 x 10−2 s−1 ) = (-115000 J/mol / (8.31 x 342 K ) + ( 115000 J/mol / (8.31 x 298 K )

ln(k2/ 3.00 x 10−2 s−1 ) = 5.97

So

k2 = e5.97 x 3.00 x 10−2 s−1

= 11.75 s−1

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