## Test 3 #5

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

Alexia Joseph 2B
Posts: 56
Joined: Thu Jul 27, 2017 3:01 am

### Test 3 #5

Given the instantaneous rate of reaction is 1.43 * 10^-2, and the initial mass of each reactant is 0.6 confined to a 750 mL vessel, how do you find the rate constant?

The rate law is rate = k [NO]^2 [O2]

Paula Sing 1J
Posts: 36
Joined: Fri Sep 29, 2017 7:06 am

### Re: Test 3 #5

First you need to solve for the molarities of NO and O2. You are given the weight in grams of each so you divide by their respective molar masses to get moles of each compound then you divide each by .75L to make the values a concentration in molarity. You would then plug in these values you have into the Rate law equation you have and solve for k.