N2 + 3H2 → 2NH3

How many grams of hydrogen, H2, are necessary to react completely with 50.0 g of nitrogen, N2?

5.4 g

28.0 g

2.0 g

10.7 g

10.7 g of H₂. Last option

Explanation:

The reaction shows that 1 mol of N₂ reacts with 3 moles of hydrogen to produce ammonia.

Let's make a rule of three with the reactant, to find the relation.

We need to convert the mass of N₂ to moles

50 g / 28g/mol = 1.78 moles

The equation is: N₂ + 3H₂ → 2NH₃

Ratio is 1:3

1 mol of N₂ reacts with 3 moles of hydrogen to produce ammonia

Therefore 1.78 moles will react with (1.78 . 3 ) / 1 = 5.36 moles

We convert the moles to mass to find out the answer

5.36 mol . 2g / 1 mol = 10.7 g

it is the most commonly accepted one

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.