Types of Reactions and Stoichiometry Review

In stoichiometry problems, usually the first thing you do when starting the calculations is

• convert given quantities to masses

• convert given quantities to volumes

• convert given quantities to moles

• convert to wanted moles using mole ratio

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

• competing side reactions

• impure reactants present

• loss of product during purification

• conservation of mass

What type of reaction is recognized by a single element and a compound?

• Combustion reaction

• Combination reaction

• Single replacement reaction

• Decomposition reaction

What type of reaction is recognized by a single product?

• Combustion reaction

• Combination reaction

• Single replacement reaction

• Decomposition reaction

What type of reaction is recognized by a single reactant?

• Combustion reaction

• Combination reaction

• Single replacement reaction

• Decomposition reaction

What type of reaction is recognized by the two reactants being aqueous solutions?

• Double replacement reaction

• Combination reaction

• Single replacement reaction

• Decomposition reaction

For the complete combustion of a hydrocarbon the products will always be ...

• Carbon monoxide and water

• carbon and water

• carbon dioxide and water

• carbonate and water

Which of the following is the correct, balanced equation for the decomposition of Calcium Oxide into its elements?

• Ca₂O(s) → Ca(s) + O₂(g)

• 2CaO(s) → 2Ca(s) + O₂(g)

• CaO₂(s) → Ca(s) + O₂(g)

• CaO(s) → Ca(s) + O₂(g)

Which of the following is correct for iron(III) is placed in copper(II) chloride?

• Fe(s) + CuCl₂(aq) → Cu(s) + FeCl₂(aq)

• Fe(s) + 2CuCl(aq) → 2Cu(s) + FeCl₂(aq)

• 2Fe(s) + 3CuCl₂(aq) → 3Cu(s) + 2FeCl₃(aq)

• 3Fe(s) + 2CuCl₂(aq) → 2Cu(s) + 3FeCl₃(aq)

The reason chemical equations are balanced is

• to satisfy the Law of Conservation of Mass.

• to satisfy the Law of Definite Proportions.

• to be prepared for stoichiometry.

• to satisfy the Law of Multiple Proportions.