## 7A.9

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

Ami_Pant_4G
Posts: 106
Joined: Sat Aug 24, 2019 12:17 am

### 7A.9

Dinitrogen pentoxide, N2O5, decomposes by a first-order reaction. What is the initial rate of decomposition of N2O5 when 3.45 g of N2O5 is confined in a container of volume 0.750 L and heated to 65 C? For this reaction, k= 5.23x10^23 s^-1 in the rate law (for the rate of decomposition of N2O5).

Can someone please explain how to solve this problem? thanks in advance.

Aliya Jain 2B
Posts: 101
Joined: Wed Sep 11, 2019 12:16 am

### Re: 7A.9

calculate the mols of N2O5 present, and multiply it by the reaction rate.

Brittney Hun 2C
Posts: 104
Joined: Wed Sep 11, 2019 12:15 am

### Re: 7A.9

First, convert the grams of N2O5 to mols and divide by the liters to get the molarity. You should get 0.0426M and then you just multiply it by the rate to get the second order reaction.

Niharika 1H
Posts: 50
Joined: Thu Jul 25, 2019 12:16 am

### Re: 7A.9

Convert dinitrogen pentoxide to moles, and then divide by the volume to get the molarity of N2O5. Plug this into the first order rate reaction.

Nohemi Garcia 1L
Posts: 103
Joined: Fri Aug 02, 2019 12:15 am

### Re: 7A.9

For this problem just use the first order equation, Rate=k[A]. Just find the concentration of N2O5 by converting the grams into moles, and then placing it over the amount in liters. Finally, all you have to do is multiply the k given with the concentration.

504939134
Posts: 103
Joined: Wed Sep 18, 2019 12:21 am

### Re: 7A.9

You first get the concentration by finding the Molar mass of N2O5 which is 108g, you then use the formula C=m/M*V and plug in the values they gave you in the problem.