## Test #3 Q3

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

nelms6678
Posts: 53
Joined: Fri Sep 29, 2017 7:07 am

### Test #3 Q3

The rate of AB4 gas consumption in this Rxn is constant throughout and is given as 0.400M/s/ If your rxn vessel starts with 0.15M of B2C, how long will it take to get to 30.00M of B2C?
AB4(g) + C2(g)---> AC2(g) + B2C(g)

Can someone walk me through this, what do you do after you balance the equation?

Lauren Seidl 1D
Posts: 51
Joined: Fri Sep 29, 2017 7:06 am

### Re: Test #3 Q3

When you balance the equation, you should get AB4(g) + 2 C2(g) ---> AC2(g) + 2 B2C(g). Because the rate of the reaction is constant, we can use the equation rate = (change in concentration)/(change in time). You must multiply the rate by 2 because there are two moles of B2C produced for each mole of AB4 consumed. This would give you 0.800 M/s = (30.00 M - 0.15 M)/time. Solving for time, you would get 37.3 seconds.

RohanGupta1G
Posts: 34
Joined: Sat Jul 22, 2017 3:00 am

### Re: Test #3 Q3

The key is you need to remember to balance the equation. Then you can use the integrated rate law to solve for time.

Justin Lai 1C
Posts: 50
Joined: Fri Sep 29, 2017 7:04 am

### Re: Test #3 Q3

When we use the (change in concentration)/(change in time) equation does that mean that it is 1st order?