AP Chemistry : Combustion

Study concepts, example questions & explanations for AP Chemistry

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Example Questions

Example Question #1 : Reactions And Equilibrium

What is the balanced equation when heptane is combusted?

Possible Answers:

C3H8 + 5 O2 → 4 H2O + 3 CO2

C7H16 + 11 O2 → 8 H2O + 7 CO2

C7H16 + O2 → H2O + CO2

2 C7H14 + 5 O2 → 3 H2O + 6 CO2

C5H12 + 8 O2 → 6 H2O + 5 CO2

Correct answer:

C7H16 + 11 O2 → 8 H2O + 7 CO2

Explanation:

Heptane: C7H16. Combustion is when a molecule reacts with O2 and the products are CO2 and H2O. Balancing gives 7 CO2, 8 H2O, 1 heptane, and 11 O2

Example Question #1 : Reaction Types

Which of the following reactions has the most exothermic heat of reaction?

Possible Answers:
The combustion of isobutane
The combustion of propane
The combustion of butane
The combustion of isopropane
The combustion of methane
Correct answer: The combustion of butane
Explanation:

The longer the hydrocarbon chain, the greater the amount of combustion products (CO2 and H20) generated. Branched molecules such as isopropane and isobutane are more difficult to combust than their straight-chain counterparts.

Example Question #2 : Reactions And Equilibrium

Which of the following conditions would describe a combustion reaction?

Possible Answers:

Exothermic with a positive \(\displaystyle \Delta H\)

Endothermic with a positive \(\displaystyle \Delta H\)

Exergonic with a positive \(\displaystyle \Delta H\)

Endergonic with a negative \(\displaystyle \Delta H\)

Exothermic with a negative \(\displaystyle \Delta H\)

Correct answer:

Exothermic with a negative \(\displaystyle \Delta H\)

Explanation:

An exothermic reaction will have a negative \(\displaystyle \Delta H\) value, indicating that it releases heat. Conversely, an endothermic reaction will have a positive \(\displaystyle \Delta H\) value, indicating a consumption of heat.

A combustion reaction releases heat; thus it must have a negative \(\displaystyle \Delta H\) value and be exothermic.

Exergonic reactions have a negative \(\displaystyle \Delta G\) value, indicating spontaneity, while endergonic reactions are non-spontaneous. While most combustion reactions will be non-spontaneous, it is impossible to draw this conclusion for certain without knowing more about the reaction. The only thing we know for certain is that heat is released, and the reaction is exothermic.

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