Question

How many grams of NH3 are required to produce 4.65 g of HF

Answer 1

1.32g

Step-by-step explanation:

Given parameters:

Mass of HF = 4.65g

Unknown:

Mass of NH₃ = ?

Solution:

We need to know the reaction equation first of all. The reaction that will produce HF involves;

2NH₃ + 5F₂ → N₂F₄ + 6HF

Now that we know the reaction equation;

Find the number of moles of the HF;

Number of moles =
`(mass)/(molar mass)`

Molar mass of HF = 1 + 19 = 20g/mol

Number of moles =
`(4.65)/(20)` = 0.23mole

From the balanced reaction equation;

6 moles of HF is produced from 2 moles of NH₃

0.23 moles of HF will be produced from
`(0.23 x 2)/(6)` = 0.08moles

Now we find the mass of NH₃

Mass of NH₃ = number of moles x molar mass

Molar mass of NH₃ = 14 + 3(1) = 17g/mol

Mass of NH₃ = 0.08 x 17 = 1.32g