Stoichiometry and Chemical Equations 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 NOT a step in determining the formula of a hydrate?

Question 2 2. What is the actual yield?

Question 3 3. What is theoretical yield?

Question 4 4. What is the hydrate formula when there are 0.02 moles BaCl2 and 0.04 moles H2 O?

Question 5 5. Determine the percent yield if the theoretical yield is 20 g and the actual yield is 15 g.

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Question 6 6. What is the empirical formula of a compound containing (by mass) 36.5% sulfur and 63.5% iron?

Question 7 7. What is meant by the term molar volume?

Question 8 8. What does the empirical formula show?

Question 9 9. At STP, how much space (in liters) will 0.750 moles of argon gas occupy?

Question 10 10. Given a balanced equation involving A and B, which set of conversions must you make to change mass A to mass B?

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

Question 12 12. How do you determine the amount of product made?

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

Question 14 14.

Choose the correctly balanced equation for the following reaction:

Potassium + water → potassium hydroxide + hydrogen gas

Question 15 15. Which of the following mole ratio is NOT appropriate to the equation 6CO2+ 6H2 O = C6 H12 O6+ 6O2?

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Question 16 16. In the formula MgSO4 nH2 O, what does the n before the H2 O stand for?

Question 17 17. What is a limiting reactant?

Question 18 18. What is the difference between a hydrate and an anhydrate?

Question 19 19. How is mass of a substance connected to its amount in mole(s)?

Question 20 20. Select the most suitable definition for stoichiometry.

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Question 21 21. 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 22 22. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

Question 23 23. What is a coefficient?

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.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

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Question 26 26. How is percent yield calculated?

Question 27 27. If there are three moles of H2 O for every one mole of LiClO4, then what is the hydrate formula?

Question 28 28. How many moles of N2 are needed to produce 18 moles NH3 in the reaction N2 + 3H2 = 2NH3?

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

Question 30 30. What is the volume of 2 moles of a gas at 300K and 1.25atm?

Stoichiometry and Chemical Equations 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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