Question

Based on the following balanced equation- How many grams of zinc oxide could be generated from 1.75 miles of zinc sulfide assuming there was excess oxygen?

C = 12.01, O = 16.00, Zn = 65.38 (g/mol)

Answer 1

mass of ZnO = 95.62 g

Step-by-step explanation:

Balanced chemical equation

2ZnS + 3O₂ → 2ZnO + 2SO₂

Given data from eq.

moles of zinc sulfide = 2 mol

moles of zinc oxide = 2 mol

mass of zinc oxide = ?

Given moles of zinc sulfide = 1.75 mol

Solution

1st we will find out the mole ratio of zinc sulfide and zinc oxide from balanced chemical equation

ZnS : ZnO

2 : 2

2/2 : 2/2

1 : 1

given number of moles of zinc sulfide = 1.75 mol

So we can find out moles (x) of ZnO needed for 1.75 mol of zinc sulfide

from the balanced chemical equation the mole ratios are:

1 : 1

1.75 : x

Cross multiply these ratios

1 × 1.175 = 1x

1.175 = 1 x

x = 1.175 mol

Now we will find out the mass of ZnO

mass = moles × molar mass

mass of ZnO = 1.175 mol × 81.38 g/mol

mass of ZnO = 95.62 g