Question

I really don't understand how to do this.
Using the Haber process to create ammonia from nitrogen and hydrogen gases, you need to manufacture 1000 liters of ammonia gas. How many liters of hydrogen gas will be consumed in the process?

Answer 1

N + 4H = NH4 you might have to apply PV=nRT @stp to do the second part. 22.4L at STP per mole of anything.

Answer 2

im still super lost.

Answer 3

the equation is wrong:
\[N_2 + 3H_2 \rightarrow 2NH_3\]
ammonia is NH3, the ammonium ion is (NH4)+1. Each time you make 2L of NH3, you'll use 3L of H2. To make 1000L of NH3, you'll use 1.5 times that amount of H2. The balanced reaction tells you the ratios of stuff you'll use

Answer 4

A key fact you'll need to completely understand what JFraser is saying (which is entirely correct and to the point) is Avogadro;'s Law: the number of atoms or molecules in a gas is proportional to the volume of the gas.

Hence, the chemical equation tells you 1 nitrogen (N2) molecule combines with 3 hydrogen (H2) molecules to give you 2 ammonia (NH3) molecules. Which means you need 3 hydrogen molecules for every 2 ammonia molecules you want to form.

Now comes Avogadro's Law: since the number of atoms or molecules is proportional to the volume, you also know that you need 3 liters of hydrogen gas for every 2 liters of ammonia gas you want to form. Since you want 1000 L of ammonia gas, you'll need 3/2 * 1000 = 1500 L of hydrogen gas.

One additional math trick I used there is proportions, which you probably studied in algebra 1. That is, I'm solving this proportion problem: if x : 1000 is to be the same proportion as 3:2, what is x? Answer 1500.