Solution Found!

Solved: Explain why reactions with large equilibrium

Chapter 14, Problem 34P

(choose chapter or problem)

Get Unlimited Answers
QUESTION:

Explain why reactions with large equilibrium constants, such as the formation of rust \(\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right)\), may have very slow rates.

Questions & Answers

QUESTION:

Explain why reactions with large equilibrium constants, such as the formation of rust \(\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right)\), may have very slow rates.

ANSWER:

Step 1 of 2

Equilibrium constant can be expressed as the ratio of forward constant to the rate of backward rate constant for the reverse reaction. It is a constant for specific reactions at specific temperatures.

It can be expressed as follows;

                                                               

 and  are the rate constants.

Add to cart


Study Tools You Might Need

Not The Solution You Need? Search for Your Answer Here:

×

Login

Login or Sign up for access to all of our study tools and educational content!

Forgot password?
Register Now

×

Register

Sign up for access to all content on our site!

Or login if you already have an account

×

Reset password

If you have an active account we’ll send you an e-mail for password recovery

Or login if you have your password back