#
**Problem**: Given that N2O4 is 2nd order for the reaction: N2O4 → 2 NO2, if a reaction started with 0.75 M N2O4, what is the half-time when the rate constant is 0.50 min-1 M-1 A. 1.33 minB. 2.25 minC. 0.50 minD. 2.67 minE. 10.3 min

###### FREE Expert Solution

We’re being asked to **calculate the half-life **of a second-order reaction with a rate constant of 0.50 min^{-1} M^{-1} initially at 0.75 M

Recall that ** half-life (t_{1/2})** is the time needed for the amount of a reactant to decrease by 50% or one-half. The half-life of a second-order reaction is given by:

$\overline{){{\mathbf{t}}}_{\mathbf{1}\mathbf{/}\mathbf{2}}{\mathbf{=}}\frac{\mathbf{1}}{\mathbf{k}{\mathbf{\left[}\mathbf{A}\mathbf{\right]}}_{\mathbf{0}}}}$

where:

**k** = rate constant

**[A] _{0}** = initial concentration

###### Problem Details

Given that N_{2}O_{4} is 2nd order for the reaction: N_{2}O_{4} → 2 NO_{2, }if a reaction started with 0.75 M N_{2}O_{4}, what is the half-time when the rate constant is 0.50 min^{-1} M^{-1}

A. 1.33 min

B. 2.25 min

C. 0.50 min

D. 2.67 min

E. 10.3 min

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Integrated Rate Law concept. You can view video lessons to learn Integrated Rate Law Or if you need more Integrated Rate Law practice, you can also practice Integrated Rate Law practice problems .

What is the difficulty of this problem?

Our tutors rated the difficulty of
*
Given that N2O4 is 2nd order for the reaction: N2O4 → 2 NO2,...
*
as medium difficulty.