Question

What is the theoretical yield of bismuth when 32.53 g of Bi2O3 reacts with excess carbon as shown below? Bi2O3 + C(s) => Bi(s) + CO(g) (not balanced)

Answer 1

In balanced reaction,

Number of atoms on either side of reaction are same.

Thus, balanced reaction is:

Bi₂O₃ (s) + 3C(s) 2Bi (s) + 3CO (g)

Molar mass of Bi₂O₃ = 465.96 g/mol

Mass of Bi₂O₃ = 32.53 g

Thus, Moles of Bi₂O₃ = mass/ molar mass = 32.53g/(465.96 g/mol) = 0.0698 mol

From reaction, 1 mol of Bi₂O₃ reacts to produce 2 mol of Bi

Thus, 0.0698 mol of Bi₂O₃ reacts to produce 0.0698 mol * 2 = 0.1396 mol of Bi

Molar mass of Bi = 208.98 g/mol

Thus, mass of Bi produced = mole *Molar mass = 208.98g/mol * 0.1396 mol = 29.18 g

Thus, theoretical yield is 29.18 g