1.326 grams of NH3 are required to produce 4.65 g of HF.
Step-by-step explanation:
Balanced chemical reaction is written first to know the number of moles taking part in original reaction.
NH3 +3 F2 ⇒3 HF + NF3
Given:
mass of HF = 4.65
First the number of moles of HF in 4.65 grams is calculated by using the formula:
number of moles (n) = [tex]\frac{mass}{atomic mass of 1 mole}[/tex]
atomic mass of HF = 20 grams/mole
putting the values in the above equation number of moles can be found.
n = [tex]\frac{4.65}{20}[/tex]
= 0.235 moles of HF are given.
From the equation it can be said that:
1 mole of NH3 reacts to form 3 moles of HF
so, x moles of NH3 would react to form 0.235 moles of HF
[tex]\frac{3}{1}[/tex] = [tex]\frac{0.235}{x}[/tex]
3x = 0.235
x = [tex]\frac{0.235}{3}[/tex]
x = 0.078 moles of NH3 is required.
The moles are converted to mass by applying the formula:
mass = atomic mass X number of moles (atomic mass of NH3 = 17 grams/mole)
putting the values in the formula
mass = 17 X 0.078
mass = 1.326 grams
