## 7A.1

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

Payton Kammerer 2B
Posts: 49
Joined: Tue May 01, 2018 3:00 am

### 7A.1

7A.1 Complete the following statements relating to the production of ammonia by the Haber process, for which the overall reac- tion is N2(g) 1 3 H2(g) S 2 NH3(g). (a) The rate of consumption of N2 is ______________ times the rate of consumption of H2. (b) The rate of formation of NH3 is ________________ times the rate of consumption of H2. (c) The rate of formation of NH3 is ________________ times the rate of consumption of N2.

Is this just supposed to be a comparison of stoichiometric coefficients? I guess I'm just confused as to how this relates to what we have learned, and I'm worried that I've oversimplified the reason for the answer being what it is. Is there a more complex explanation that uses rate=k[][]?

christabellej 1F
Posts: 109
Joined: Sat Aug 17, 2019 12:17 am

### Re: 7A.1

Yes, it just has to do with stoichiometric coefficients.For part a for example, the rate of consumption of N2 is 1/3 times the rate of consumption of H2 because H2 is consumed three times as much as N2.

Megan Vu 1J
Posts: 101
Joined: Thu Jul 25, 2019 12:15 am

### Re: 7A.1

This is a comparison of the stoichiometric coefficients which relates to kinetics.
For example, the first part in a, you should compare N2 and H2 to each other in the chemical equation.
Since it takes 3 moles of H2 to make 1 mole of N2, then you should be able to multiply H2 by 1/3 to get 1 mole of N2.
Thus, the answer would be 1/3. You should compare for all of the parts.

Emily Vainberg 1D
Posts: 102
Joined: Sat Jul 20, 2019 12:15 am

### Re: 7A.1

I didn't even use the formula for this question, I just looked at the equation. when you compare the reactants, one mole of NH3 is used for every 3 moles of H2. This means that for part a) The rate of consumption of N2 is (1/3) times the rate of consumption of H2.