MCQs

Hydrogen is the limiting reactant because 9 moles are required. Six moles of hydrogen produce four moles of ammonia.

Na₂SO₄ contains two sodium ions per formula unit. Therefore, 0.5 mole gives one mole of Na⁺ ions.

Glucose contains six carbon atoms per molecule. Therefore, 0.5 mole of carbon atoms corresponds to 0.5 ÷ 6 = 0.083 mole of glucose.

Each NH₃ molecule contains three hydrogen atoms; therefore one mole of NH₃ contains three moles of hydrogen atoms.

Forty-eight grams of magnesium equal two moles, producing two moles of MgO. The mass becomes 80 g.

One mole occupies 22.4 dm³ at STP, so two moles occupy 44.8 dm³.

One mole of nitrogen produces two moles of nitrogen dioxide. Therefore, 0.5 mole yields one mole.

One mole always contains 6.022 × 10²³ elementary particles.

The balanced equation directly provides the ratio.

This represents 0.5 mole of water. Half of 18 g equals 9 g.

Stoichiometric calculations depend entirely upon balanced mole ratios.

Each mole of sucrose contains 12 moles of carbon atoms. Therefore, two moles contain 24 moles.

The mole ratio Al:Cl₂ is 2:3. Therefore, 5 moles of aluminium require 7.5 moles of chlorine.

Every mole contains the same number of molecules, although the number of atoms differs.

Stoichiometric coefficients indicate mole relationships among reactants and products.

One mole of Fe₂O₃ produces two moles of iron. Two × 55.85 g equals 111.7 g.

Each formula unit contains three ions. Therefore, one mole contains three times Avogadro's number of ions.

Hydrogen and water have a 1:1 mole relationship in the balanced equation.

Half a mole contains half of Avogadro's number of molecules.