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Stoichiometry: Help and Review 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. 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 2 2. What is the hydrate formula when there are 0.02 moles BaCl2 and 0.04 moles H2 O?

Question 3 3. What is the difference between a hydrate and an anhydrate?

Question 4 4. What is a coefficient?

Question 5 5. Which of the following calculations is NOT needed to determine the empirical formula?

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Question 6 6. How many moles of solute are in a 0.50 L solution of 3.0 molarity?

Question 7 7. The starting point of a stoichiometric problem is _____.

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

Question 9 9. How is a mole ratio used?

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

Question 12 12. What is the empirical formula of a compound containing (by mass) 36.5% sulfur and 63.5% iron?

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. What is the volume of 2 moles of a gas at 300K and 1.25atm?

Question 15 15. 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 16 16. At STP, how much space (in liters) will 0.750 moles of argon gas occupy?

Question 17 17. Given a balanced equation involving A and B, which set of conversions must you make to change mass A to mass B?

Question 18 18. What does the empirical formula show?

Question 19 19. What is the percent composition of Cu₂S?

Question 20 20. 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?

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Question 21 21. In the formula MgSO4 nH2 O, what does the n before the H2 O stand for?

Question 22 22. How do you determine the amount of product made?

Question 23 23. What is a limiting reactant?

Question 24 24.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

Question 25 25. 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 26 26. Which of the following mole ratio is NOT appropriate to the equation 6CO2+ 6H2 O = C6 H12 O6+ 6O2?

Question 27 27. Conservation of matter means that:

Question 28 28. How is percent yield calculated?

Question 29 29. What is meant by the term molar volume?

Question 30 30. Which of the following equations is balanced?

Stoichiometry: Help and Review 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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