Overview of Stoichiometry 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. How many moles of N2 are needed to produce 18 moles NH3 in the reaction N2 + 3H2 = 2NH3?

Question 2 2. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

Question 3 3. What is meant by the term molar volume?

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

Question 5 5. Conservation of matter means that:

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Question 6 6. In the formula MgSO4 nH2 O, what does the n before the H2 O stand for?

Question 7 7. Which of the following mole ratio is NOT appropriate to the equation 6CO2+ 6H2 O = C6 H12 O6+ 6O2?

Question 8 8. How is mass of a substance connected to its amount in mole(s)?

Question 9 9. 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 10 10.

Choose the correctly balanced equation for the following reaction:

Potassium + water → potassium hydroxide + hydrogen gas

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Question 11 11. How do you determine the amount of product made?

Question 12 12.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

Question 13 13. What is the percent composition of H₂SO₃?

Question 14 14. Which of the following equations is balanced?

Question 15 15. The starting point of a stoichiometric problem is _____.

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Question 16 16. Determine the actual yield if the theoretical yield is 12 g and the percentage yield is 90%.

Question 17 17. How many moles of solute are in a 0.50 L solution of 3.0 molarity?

Question 18 18. Where do you look to find the molar ratio?

Question 19 19. What is the hydrate formula when there are 0.02 moles BaCl2 and 0.04 moles H2 O?

Question 20 20. What is the percent composition of Cu₂S?

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Question 21 21. What is NOT a step in determining the formula of a hydrate?

Question 22 22. What is a coefficient?

Question 23 23. 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 24 24. What does the empirical formula show?

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

Question 27 27. What is theoretical yield?

Question 28 28. What is the actual yield?

Question 29 29. 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 30 30. Given a balanced equation involving A and B, which set of conversions must you make to change mass A to mass B?

Overview of Stoichiometry 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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