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Stoichiometry & Chemical Equations: AP Chemistry Lesson Plans Chapter Exam

Exam Instructions:

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

Page 1

Question 1 1. How is mass of a substance connected to its amount in mole(s)?

Question 2 2.

Choose the correctly balanced equation for the following reaction:

Potassium + water → potassium hydroxide + hydrogen gas

Question 3 3. Which of the following equations is balanced?

Question 4 4. Given a balanced equation involving A and B, which set of conversions must you make to change mass A to mass B?

Question 5 5. You conduct an experiment that requires the creation of an ammonia solution. You do this by reacting 50.0 L of nitrogen gas with excess hydrogen gas at STP to create ammonia gas using the Haber process given by the following reaction: N2 (g) + 3H2 (g) → 2NH3 (g). Assuming the reaction had 100% yield, you then bubble the ammonia into 5.0 L of water. What is the molarity of the resulting ammonia solution?

Page 2

Question 6 6. Which of the following calculations is NOT part of determining the empirical formula?

Question 7 7. 3.9 g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

Question 8 8. What is the empirical formula of a compound containing (by mass) 36.5% sulfur and 63.5% iron?

Question 9 9. What is a coefficient?

Question 10 10. At STP, how much space (in liters) will 0.750 moles of argon gas occupy?

Page 3

Question 11 11. What is the percent composition of Cu₂S?

Question 12 12. Conservation of matter means that:

Question 13 13. How many moles of Na are needed to produce 15 moles of NaCl in the reaction 2Na + Cl2 → 2NaCl?

Question 14 14. Say you take a reactant A and calculate the amount of moles of another reactant B required to use up all of A. How do you know which of two reactants is the limiting one?

Question 15 15. If 2.5 moles of zinc react with 6.0 moles of hydrochloric acid in the equation Zn + 2HCl = ZnCl2 + H2, what is the limiting reactant?

Page 4

Question 16 16. What is the actual yield?

Question 17 17. If 1.605 kg of mercury are used in the reaction 2Hg + O2 --> 2HgO, what is the mass of HgO, in kilograms, that are produced?

Question 18 18. What is the hydrate formula when there are 0.02 moles BaCl2 and 0.04 moles H2 O?

Question 19 19. What is NOT a step in determining the formula of a hydrate?

Question 20 20. How many moles of solute are in a 0.50 L solution of 3.0 molarity?

Page 5

Question 21 21. Where do you look to find the molar ratio?

Question 22 22.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

Question 23 23. How is a mole ratio used?

Question 24 24. Determine the percent yield if the theoretical yield is 20 g and the actual yield is 15 g.

Question 25 25. How many moles of N2 are needed to produce 18 moles NH3 in the reaction N2 + 3H2 → 2NH3?

Page 6

Question 26 26. What is meant by the term molar volume?

Question 27 27. What is the difference between a hydrate and an anhydrate?

Question 28 28. If there are three moles of H2 O for every one mole of LiClO4, then what is the hydrate formula?

Question 29 29. Which of the following mole ratio is NOT appropriate to the equation 6CO2+ 6H2 O → C6 H12 O6+ 6O2?

Question 30 30. How is percent yield calculated?

Stoichiometry & Chemical Equations: AP Chemistry Lesson Plans Chapter Exam Instructions

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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