AP Chemistry: Stoichiometry and Chemical Equations: Homework Help 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!

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Question 1 1. What is the difference between a hydrate and an anhydrate?

Question 2 2. What is meant by the term molar volume?

Question 3 3. What is the actual yield?

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. What is a limiting reactant?

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Question 6 6. How many moles of Na are needed to produce 15 moles of NaCl in the reaction 2Na + Cl2 → 2NaCl?

Question 7 7. What is the percent composition of H₂SO₃?

Question 8 8.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

Question 9 9. How do you determine the amount of product made?

Question 10 10. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

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Question 11 11. Determine the percent yield if the theoretical yield is 20 g and the actual yield is 15 g.

Question 12 12. How is mass of a substance connected to its amount in mole(s)?

Question 13 13. How many moles of solute are in a 0.50 L solution of 3.0 molarity?

Question 14 14. What is NOT a step in determining the formula of a hydrate?

Question 15 15. How is percent yield calculated?

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Question 16 16. 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?

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. Which of the following calculations is NOT needed to determine the empirical formula?

Question 19 19. Select the most suitable definition for stoichiometry.

Question 20 20. If 4.0 moles of HCl react with 5.0 moles of NaOH to make NaCl and H2 O in the equilibrium reaction HCl+ NaOH = NaCl + H2 O, what is the limiting reactant?

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Question 21 21. How is a mole ratio used?

Question 22 22. How many moles of N2 are needed to produce 18 moles NH3 in the reaction N2 + 3H2 → 2NH3?

Question 23 23. Conservation of matter means that:

Question 24 24. 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?

Question 25 25. At STP, how much space (in liters) will 0.750 moles of argon gas occupy?

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Question 26 26. Which of the following mole ratio is NOT appropriate to the equation 6CO2+ 6H2 O → C6 H12 O6+ 6O2?

Question 27 27. What is a coefficient?

Question 28 28. What is the hydrate formula when there are 0.02 moles BaCl2 and 0.04 moles H2 O?

Question 29 29. Which of the following equations is balanced?

Question 30 30. What is the percent composition of Cu₂S?

AP Chemistry: Stoichiometry and Chemical Equations: Homework Help 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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