In 1909 fritz haber discovered the workable conditions under which nitrogen, n2(g), and hydrogen, h2(g), would combine using to produce ammonia. the conditions included medium temperature (~500oc), very high pressure (~351kpa), and an iron catalyst. the reaction is represented by the equation: n2(g) + 3h2(g) → 2nh3(g) how many grams of nitrogen are needed to produce 100 grams of ammonia gas?

Answer : 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.

Solution : Given,

Mass of = 100 g

Molar mass of = 27 g/mole

Molar mass of = 28 g/mole

First we have to calculate moles of .

The given balanced chemical reaction is,

From the given reaction, we conclude that

2 moles of produced from 1 mole of

3.7 moles of produced from of

Now we have to calculate the mass of .

Mass of = Moles of × Molar mass of

Mass of = 1.85 mole × 28 g/mole = 51.8 g

Therefore, 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.