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AP®ChemistryCollege BoardExam QuestionsUnit 4: Chemical ReactionsTypes of Chemical Reactions

Types of Chemical Reactions (College Board AP® Chemistry): Exam Questions

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Types of Chemical Reactions

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Types of Chemical Reactions

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1a1 mark

Aqueous solutions of silver nitrate (AgNO3) and potassium chromate (K2CrO4) are mixed, resulting in the formation of a red precipitate. The chemical equation for this reaction is:

2AgNO3 (aq) + K2CrO4 (aq) → Ag2CrO4 (s) + 2KNO3 (aq)

Identify the type of reaction represented by this equation.

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1b1 mark

Write the net ionic equation for the reaction in part (a).

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1c1 mark

Predict whether the mass of solid formed would increase, decrease, or remain the same if the concentration of AgNO3​ (aq) were increased. Justify your answer.

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1d1 mark

Describe how you could experimentally confirm that a chemical reaction has occurred when these two solutions in part (a) are mixed.

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2a1 mark

Ethanol (C2H5OH) burns in oxygen to produce carbon dioxide and water:

C2H5OH (l) + 3O2 (g) → 2CO2 (g) + 3H2O (g)

Identify the type of reaction represented by this equation.

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2b1 mark

Explain why the reaction produces more energy when the products are only carbon dioxide (CO2) and water (H2O) compared to other possible products.

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2c2 marks

A chemist has a rigid 15.0 L container of oxygen gas O2 (g) at a pressure of 0.50 atm and a temperature of 298 K. Using the ideal gas law:

i) Calculate the number of moles of oxygen gas in the container.

ii) Determine the number of moles which is enough to completely combust 0.50 moles of ethanol.

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3a2 marks

A solution of sodium bicarbonate (NaHCO3​) reacts with hydrochloric acid (HCl) in water, as shown in the equation:

HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2CO3 (aq)

Identify the acid and the base in the reaction between HCl and NaHCO3​.

Explain your reasoning based on the transfer of protons.

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3b2 marks

Explain whether the reaction between HCl and NaHCO3​ also involves oxidation or reduction.

Support your answer by analyzing the oxidation numbers of the key species involved.

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1a2 marks

Iron(III) oxide (Fe2O3​) reacts with carbon monoxide (CO) in a blast furnace to produce molten iron (Fe) and carbon dioxide (CO2​):

Fe2O3 (s) + 3CO (g) → 2Fe (l) + 3CO2 (g)

Identify the species that is oxidized and the species that is reduced. Justify your answer.

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1b2 marks

Calculate the mass of CO consumed and the mass of Fe produced when 32.0 g of Fe2O3​ reacts completely.

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2a1 mark

Hydrogen peroxide (H2O2) reacts with iron(III) ions (Fe3+) in acidic solution to form chromate (Fe2+) and oxygen gas (O2) according to the equation:

2Fe3+ (aq) + H2O2 (l) → 2Fe2+(aq) +O2 (g) + 2H+ (aq)

Write the oxidation and reduction half equations for this reaction.

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2b1 mark

Hydrogen peroxide reacts with iodide ions, I-, in acidic solution to produce iodine and water.

H2O2 (aq) + 2I- (aq) + 2H+ (aq) → I2 (aq)+ 2H2O (l)

Explain why this reaction is classified as an oxidation-reduction reaction. Identify the species that is oxidized and the species that is reduced. Support your answer using oxidation numbers.

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3a2 marks

Sulfuric acid (H2SO4) is a diprotic acid that reacts with calcium hydroxide (NaHCO3) in aqueous solution.

i) Write the balanced equation for this reaction.

ii) Write the net ionic equation for the reaction that demonstrates that neutralization has occurred.

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3b2 marks

If 50.0 mL 0.200 M H2SO4​ reacts completely with NaHCO3, calculate the volume of gas produced at 25 ∘C and 1.00 atm.

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