Question

How many grams of H2 are needed to produce 13.54 g of NH3?

Answer 1

The balanced chemical for the formation of NH3 from H2 is given below,

Let us first calculate the number of moles of NH3 required to produce from the mass of NH3.

The number of moles of NH3 = mass of NH3 in g / molecular weight of NH3 in g/mol

Here, mass of NH3 = 13.54 g and molecular weight of NH3 is 17 g/mol

Number of moles of NH3 = 13.54 g / 17 g/mol

= 0.796 moles

From the equation it is clear that 3 moles of H2 are required to produce 2 moles of NH3. Therefore, we can consider

2 moles of NH3 = 3 moles of H2

For, 0.796 moles of NH3 = (0.796 x 3) / 2 moles of H2

= 1.194 moles of H2

The moles of H2 can be converted to mass by using following formula.

Mass of H2 in g = number of moles of H2 x molecular weight of H2 in g/mol

Here, molecular weight of H2 = 2 g/mol

Mass of H2 in g = 1.194 mol x 2 g/mol = 2.4 g

Therefore the mass of H2 required will be 2.4 g