Answer to Question #350672 in Chemistry for Cow

Question

2. How many moles of Na2O (sodium oxide) are produced if 1.5 mol of Fe(iron) is

produced in the following reaction:

6Na + Fe2O3 - 3Na,O + 2Fe

3. If 4.3 moles of CaC2 (calcium carbonide) are used up in the reaction below, how

many grams of HO(water) are needed?

CaC2 + H20 - CaH2 +Ca(OH)?

Answer 1

Solution (2):

Balanced chemical equation:

6Na + Fe₂O₃ → 3Na₂O + 2Fe

According to stoichiometry:

When 2 mol of Fe are produced, 3 mol of Na₂O are produced.

When 1.5 mol of Fe are produced, X mol of Na₂O are produced.

Therefore,

Moles of Na₂O = X = (1.5 mol Fe) × (3 mol Na₂O / 2 mol Fe) = 2.25 mol Na₂O

Answer (2): 2.25 moles of Na₂O (sodium oxide) are produced.

Solution (3):

Balanced chemical equation:

CaC₂ + 2H₂O → C₂H₂ + Ca(OH)₂

According to stoichiometry:

1 mol of CaC₂ reacts with 2 mol of H₂O

Thus, 4.3 mol of CaC₂ react with:

(4.3 mol CaC₂) × (2 mol H₂O / 1 mol CaC₂) = 8.6 mol H₂O

The molar mass of water (H₂O) is 18.0 g/mol

Therefore,

Mass of H₂O = (8.6 mol H₂O) × (18.0 g H₂O / 1 mol H₂O) = 154.8 g H₂O

Answer (3): 154.8 grams of H₂O (water) are needed.