Question

In an industrial process, nitrogen is reacted with hydrogen to produce ammonia. the percent yield of this particular process is 28%. how much hydrogen is needed to produce 3.5 kg ammonia?

a) 2.5 kg
b) 6.25 kg
c) 8.75 kg
d) 12.5 kg

Answer 1

To produce 3.5 kg of ammonia, approximately 722.5 g (0.7225 kg) of hydrogen is needed.

Step-by-step explanation:

In this industrial process, the percent yield is given as 28%.

This means that only 28% of the reactants will form the desired product. To find out how much hydrogen is needed to produce 3.5 kg of ammonia, we can set up a proportion based on the balanced chemical equation:

N2 + 3H2 → 2NH3

The molar mass of ammonia (NH3) is 17.03 g/mol. So, to produce 3.5 kg (3500 g) of ammonia, we need:

(3500 g NH3) x (1 mol NH3 / 17.03 g NH3) x (3 mol H2 / 2 mol NH3) x (2.02 g H2 / 1 mol H2) = 722.5 g H2

Therefore, the answer is approximately 722.5 g of hydrogen, which is equivalent to 0.7225 kg. So, the correct option is b) 0.7225 kg.