Stoichiometry Review

When iron rusts in air, iron(III) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in

the rusting reaction?

4Fe(s) + 3O2(g) → 2Fe2O3(s)

• 1.2 mole

• 1.8 mole

• 2.4 mole

• 3.2 mole

In the reaction 2CO(g) + O2(g) → 2CO2(g), what is the ratio of moles of oxygen used to moles of CO2

produced?

• 1:1

• 2:1

• 1:2

• 2:2

The calculation of quantities in chemical equations is called

• dimensional analysis

• percent composition

• percent yield

• stoichiometry

Which conversion factor do you use first to calculate the number of grams of CO2 produced by the reaction

of 50.6 g of CH4 with O2?

1CH₄ + 2O₂ --> 1CO₂ + 2H₂O

• 44.0 g CO₂ / 2 mole CO₂

• 2 mole O₂ / 1 mole CO₂

• 16.0 g CH₄ / 1 mole CH₄

• 1 mole CH₄ / 16.0 g CH

Which of the following is NOT a reason why actual yield is less than theoretical yield?

• reaction stops before it is completed

• conservation of mass

• impure reactants that create new products

• loss of product

When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the

• minimum yield

• percent yield

• percent composition

• theoretical yield

Stoichiometry is based on the law of

• constant mole ratios

• Avogadro's constant

• conservation of mass

• conservation of energy

The first step in most stoichiometry problems is to

• balance the chemical equation

• add the coefficients of the reagents

• convert given quantities to masses

• convert given quantities to volume

In a chemical reaction, the mass of the products

• has no relationship to the mass of the reactants.

• is less than the mass of the reactants.

• is equal to the mass of the reactants.

• is greater than the mass of the reactants.

In every chemical reaction

• moles and liters are conserved

• mass and molecules are conserved

• moles and molecules are conserved

• mass and atoms are conserved