The isomerization reaction, A â B, is first order and the rate constant is equal to 0.027 s-1 at 500 K. Given an initial concentration of 0.14 M, calculate the concentration of A remaining at 30.0 s in mol/L.

answer

watching

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Jean KeelingLv2

13 Dec 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

For the past 10 years, the unsaturated hydrocarbon 1,3-butadiene (CH₂=CH=CH=CH₂) has ranked 38th among the 50 industrial chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene:

The isomerization of cyclobutene to 1,3-butadiene is first order and the rate constant has been measured as 2.0 x 10^-4 s^-1at 150^oC in a 0.53 L flask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150^oC with an initial pressure of 55 torr.

blackscorpion701

The reaction of NO and O₂ produces NO₂.

2 NO(g) + O₂(g) Â® 2 NO₂(g)

The reaction is second-order with respect to NO(g) and first-order with respect to O₂(g). At a given temperature, the rate constant, k, equals 6.1 Â´ 10³ M^-2s^-1. What is the rate of reaction when the initial concentrations of NO and O₂ are 0.020 M and 0.015 M, respectively?