Question

The haber process can be used to produce ammonia (nh3) from hydrogen gas (h2) and nitrogen gas (n2). the balanced equation for this process is shown below. 3h2 n2 right arrow. 2nh3 the molar mass of nh3 is 17.03 g/mol. the molar mass of h2 is 2.0158 g/mol. in a particular reaction, 0.575 g of nh3 forms. what is the mass, in grams, of h2 that must have reacted, to the correct number of significant figures? 0.1 grams 0.102 grams 0.10209 grams 0.1021 grams

Answer 1

The mass of H₂ that must have reacted is approximately 0.10209 grams.

Step-by-step explanation:

The balanced equation for the Haber process is:

N₂(g) + 3H₂(g) → 2NH₃(g)

This equation shows that for every 3 moles of H₂, 2 moles of NH₃ are formed. To find the mass of H₂ that reacted, we can use the molar mass of NH₃. The molar mass of NH₃ is 17.03 g/mol, so we can set up a proportion:

(0.575 g NH₃) / (17.03 g/mol NH₃) = (x g H₂) / (2.0158 g/mol H₂)

Solving for x gives us x ≈ 0.10209 g H₂. Therefore, the mass of H₂ that must have reacted is approximately 0.10209 grams.