Answer to Question #67063 in Physical Chemistry for Tianna

Question #67063

. The half-life for the first-order decomposition of N2O5 is 2.05 x 104 s. How long will it take for a sample of this compound to decay to 80% of its initial value?

Expert's answer

Download Answer

Learn more about our help with Assignments: Physical Chemistry

Comments

No comments. Be the first!

Leave a comment

Related Questions

1. . A first-order reaction is 60% complete at the end of 90 min, what is the value of rate constant in
2. The rate constant of a zero-order reaction is 0.2 (mol/L) hour-1. What will be the initial concentra
3. Catalyzed reactions are faster because: a. The concentrations are higher b. The temperature is hig
4. . The reaction: A → B follows first-order kinetics. The time taken for 0.8 mol of A to produce 0.6
5. 4. The rate of a reaction doubles when the concentration of one of the reactants is doubled. In te
6. 1. For a certain first order reaction, it is found that it takes 156 seconds for the concentration o
7. 100mL of oxalic acid requires35mL of 0.04 M KMnO4 to titrate it to the end point. Calculate the mol

Who Can Help Me with My Assignment

There are three certainties in this world: Death, Taxes and Homework Assignments. No matter where you study, and no matter…
How to Finish Assignments When You Can’t

Crunch time is coming, deadlines need to be met, essays need to be submitted, and tests should be studied for.…
How to Effectively Study for a Math Test

Numbers and figures are an essential part of our world, necessary for almost everything we do every day. As important…