## Finding the effect on the rate when changing the amount of reactant (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

### Finding the effect on the rate when changing the amount of reactant (test 3 #5)

The problem is:
Given: 2NO + O2 = 2NO2
The rate of the reaction was first order wrt O2, and the rate was second order wrt nitrogen monoxide.

How are you supposed to find the effect of changing the amount of oxygen/amount of nitrogen monoxide?

More specifically,

How do you find out what happens to the rate if we double the amount of oxygen or what happens if we have the amount of NO?

I know that the rate law is rate = k [NO]^2 [O2], but where do you go from here?

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

### Re: Finding the effect on the rate when changing the amount of reactant (test 3 #5)

Are you supposed to just determine it based on the rate equation, so that doubling oxygen makes the rate 1/2 slower, or halving the amount of NO makes the rate 1/4?