Question

In the following reaction, how many grams of ammonia (NH3) will produce 300 grams of N2? 4NH3 + 6NO → 5N2 + 6H2O The molar mass of ammonia is 17.0337 grams and that of nitrogen is 28.02 grams.

Answer 1

In this reaction, 4 moles NH3 produces 5 Moles of N2

1 mole NH3 = 17.0337 g
1 mole N2 = 28.02 g

Convert 300 g ammonia into moles:
\[ \frac{1 ~mol ~NH_3}{17.0337~g~ NH_3} =\frac{x~ mol NH_3}{300 ~ g ~NH_3} \implies x=17.612~ mol~NH_3\]

Now, you can find the amount of moles that will be produced in the reaction by the ratio of 4 moles NH3 produced for 5 moles of N2:
\[ \frac{4~mol ~NH_3}{17.612~mol~NH3}=\frac{5~mol~N_2}{x~ mol~N_2}\]

Once you find the amount of moles produced of N2, then covert the moles into grams using the molar mass : 1 mole N2 = 28.02 g

Answer 2

What was the final answer to this?