Question

4. Ammonia is produced by the chemical reaction of nitrogen and hydrogen. N2 (g) + 3H2(g) →→ 2NH3 (9) (A) Calculate the number of moles of hydrogen, H2, needed to react with 1.80 moles of nitrogen, N2. (5 points) (B) Calculate the grams of NH3 formed when 2.4 moles of H2 reacts completely with sufficient amount of N2. (5 points)

Answer 1

Answer:

a) No. of moles of hydrogen needed = 5.4 mol

b) Grams of ammonia produced = 27.2 g

Explanation:

$N_2 (g) + 3H_2(g) \rightarrow 2NH_3 (g)$

a)

No. of moles of nitrogen = 1.80 mol

1 mole of nitrogen reacts with 3 moles of hydrogen

1.80 moles of nitrogen will react with

                               = 1.80 × 3 = 5.4 moles of hydrogen

b)

No. of moles of hydrogen = 2.4 mol

It is given that nitrogen is present in sufficient amount.

3 moles of hydrogen produce 2 moles of $NH_3$

2.4 moles of hydrogen will produce

                              = $\frac{2}{3} \times 2.4 = 1.6\ mol\ of\ NH_3$

Molar mass of ammonia = 17 g/mol

Mass in gram = No. of moles × Molar mass

Mass of ammonia in g = 1.6 × 17

                                    = 27.2 g