Question

Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia.

N₂(g) + 3H₂(g) --> 2NH₃(g)

assume 4 molecules of nitrogen and 9 molecules of hydrogen are present.

After complete reaction, how many molecules of ammonia are produced?

How many molecules of H2 remain?

How many molecules of N2 remain?

What is the limiting reactant? hydrogen or nitrogen

Please answer all questions and explain this is due today thank you :)

Answer 1

N2(g) + 3H2(g) --> 2NH3(g)

according to balanced reaction

1 molecule N2 reacts with 3 molecules of H2

4 molecules of N2 reacts with 4 x 3 = 12 molecules of H2.

but we have only 9 molecules of H2.

so H2 is limiting reagent.

1) 3 molecules H2 gives 2 molecules of NH3

9 molecules of H2 gives 9 x 2 / 3 =6.0

molecules of ammonia formed = 6.0

2) all H2 consumed so 0 molecules of H2 remains.

3) 3 molecules of H2 reacts with 1 molecules of N2

9 molecules of H2 reacts with 9 x 1 / 3 = 3 molecules of N2

we have molecules of N2

N2 left = 4 - 3.0 - 1.0

N2 molecules left = 1.0

4) limiting reactant = H2.