AP Chemistry: Stoichiometry and Chemical Equations: Tutoring Solution 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 a coefficient?

Question 2 2. Which of the following equations is balanced?

Question 3 3. In the formula MgSO4 nH2 O, what does the n before the H2 O stand for?

Question 4 4. Determine the percent yield if the theoretical yield is 20 g and the actual yield is 15 g.

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?

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Question 6 6. How is percent yield calculated?

Question 7 7. At STP, how much space (in liters) will 0.750 moles of argon gas occupy?

Question 8 8. What is theoretical yield?

Question 9 9.

Choose the correctly balanced equation for the following reaction:

Potassium + water → potassium hydroxide + hydrogen gas

Question 10 10. How do you determine the amount of product made?

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Question 11 11. Which of the following calculations is NOT needed to determine the empirical formula?

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

Question 13 13. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

Question 14 14. What is the hydrate formula when there are 0.02 moles BaCl2 and 0.04 moles H2 O?

Question 15 15. What is meant by the term molar volume?

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Question 16 16. How many moles of Na are needed to produce 15 moles of NaCl in the reaction 2Na + Cl2 → 2NaCl?

Question 17 17. What is the percent composition of Cu₂S?

Question 18 18. How many moles of solute are in a 0.50 L solution of 3.0 molarity?

Question 19 19.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

Question 20 20. How many moles of N2 are needed to produce 18 moles NH3 in the reaction N2 + 3H2 → 2NH3?

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Question 21 21. 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 22 22. 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 23 23. The starting point of a stoichiometric problem is _____.

Question 24 24. 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 25 25. What is NOT a step in determining the formula of a hydrate?

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Question 26 26. What is a limiting reactant?

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

Question 28 28. What is the empirical formula of a compound containing (by mass) 36.5% sulfur and 63.5% iron?

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. What is the percent composition of H₂SO₃?

AP Chemistry: Stoichiometry and Chemical Equations: Tutoring Solution 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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