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

Question 2 2. At STP, how much space (in liters) will 0.750 moles of argon gas occupy?

Question 3 3. What does the empirical formula show?

Question 4 4. How is mass of a substance connected to its amount in mole(s)?

Question 5 5.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

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Question 6 6. What is the hydrate formula when there are 0.02 moles BaCl2 and 0.04 moles H2 O?

Question 7 7. How do you determine the amount of product made?

Question 8 8. Select the most suitable definition for stoichiometry.

Question 9 9. If there are three moles of H2 O for every one mole of LiClO4, then what is the hydrate formula?

Question 10 10. The starting point of a stoichiometric problem is _____.

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Question 11 11. How is a mole ratio used?

Question 12 12. 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 13 13. What is NOT a step in determining the formula of a hydrate?

Question 14 14. Determine the actual yield if the theoretical yield is 12 g and the percentage yield is 90%.

Question 15 15. 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?

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Question 16 16. What is meant by the term molar volume?

Question 17 17. What is a coefficient?

Question 18 18. What is the actual yield?

Question 19 19. What is the difference between a hydrate and an anhydrate?

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. Which of the following equations is balanced?

Question 22 22. What is a limiting reactant?

Question 23 23. Which of the following calculations is NOT needed to determine the empirical formula?

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

Question 25 25. In the formula MgSO4 nH2 O, what does the n before the H2 O stand for?

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Question 26 26. What is the empirical formula of a compound containing (by mass) 36.5% sulfur and 63.5% iron?

Question 27 27. 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 28 28. Where do you look to find the molar ratio?

Question 29 29. 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?

Question 30 30. How many moles of solute are in a 0.50 L solution of 3.0 molarity?

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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