6.10 Multiple Choice Questions

Welcome to Unit 6 AP Chemistry Multiple Choice Questions! Grab some paper and a pencil 📄 to record your answers as you go. You can see how you did on the Unit 6 Practice Questions Answers and Review sheet once you're done. Don't worry, we have tons of resources available if you get stumped 😕 on a question. And if solo study is not your thing, join a group in Hours!

Not ready to take a quiz yet? Take a look at the Intro to Unit 6

Facts about the test: The AP Chemistry exam has 60 multiple choice questions and you will be given 1 hour 30 minutes to complete the section. That means it should take you around 15 minutes to complete 10 questions. *The following questions were not written by College Board and, although they cover information outlined in the AP Chemistry Course and Exam Description, the formatting on the exam may be different.

A. Potential Energy

B. Velocity

C. Heat

D. Temperature

A. 5.39 kJ

B. 5390 kJ

C. 4.49 kJ

D. 9.88 kJ

A. 16.3 kJ

B. 43.3 kJ

C. 293 kJ

D. 2.40 kJ

A. 0.588 g

B. 36.7 g

C. 110 g

D. 1.73 g

A. The reaction will cause the surrounding's temperature to increase because the reaction is exothermic.

B. The reaction will cause the surrounding's temperature to decrease because the reaction is exothermic.

C. The reaction will cause the surrounding's temperature to increase because the reaction is endothermic.

D. The reaction will cause the surrounding's temperature to decrease because the reaction is endothermic.

A. 352.6 kJ/mol

B. -352.6 kJ/mol

C. 176.3 kJ/mol

D. -176.3 kJ/mol

A. Combusting methane

B. Freezing benzene

C. Condensing water

D. Melting wax

A. -299.4 kJ/mol

B. 149.7 kJ/mol

C. -149.7 kJ/mol

D. 299.4 kJ/mol

A. CH4 (g) + 2O2(g) -> 2H2O(g) + CO2 (g)

B. H2O (l) -> H2O (g)

C. CO2 (s) -> CO2 (g)

D. CaCO3 (s) -> CaO (s) + CO2(g)

A. The final temperature for the metal will be hotter than the initial temperature of the metal at thermal equilibrium.

B. The final temperature of the metal will be cooler than the initial temperature of the water at thermal equilibrium.

C. The average kinetic energy of the water will increase while the average kinetic energy for the metal will decrease.

D. The average kinetic energy of the metal will increase while the average kinetic energy for the water will decrease.

A. Iron (C=0.44 J/g°C)

B. Aluminum (C=0.91 J/g°C)

C. Copper (C=0.39 J/g°C)

D. Lead (C=0.13 J/g°C)

A. 11100 kJ

B. 252 kJ

C. 50.3 kJ

D. 84.0 kJ

A. More energy is released when the bonds form than energy is required to break the bonds, because the reaction is exothermic.

B. More energy is released when the bonds form than energy is required to break the bonds, because the reaction is endothermic.

C. Less energy is released when the bonds form than energy is required to break the bonds, because the reaction is exothermic.

D. Less energy is released when the bonds form than energy is required to break the bonds, because the reaction is endothermic.

A. 36°C

B. -21°C

C. 22°C

D. 51°C

A. After the combustion the temperature of the calorimeter will decrease because combustion reactions are exothermic.

B. After the combustion the temperature of the calorimeter will increase because combustion reactions are exothermic.

C. After the combustion the temperature of the calorimeter will increase because combustion reactions are endothermic.

D. After the combustion the temperature of the calorimeter will decrease because combustion reactions are endothermic.