Physical Science - 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. Determine the actual yield if the theoretical yield is 12 g and the percentage yield is 90%.

Question 2 2. What is meant by the term molar volume?

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

Question 4 4. What is theoretical yield?

Question 5 5. What is the actual yield?

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

Question 7 7. What is the percent composition of H₂SO₃?

Question 8 8. Which of the following calculations is NOT needed to determine the empirical formula?

Question 9 9. In the formula MgSO4 nH2 O, what does the n before the H2 O stand for?

Question 10 10. Select the most suitable definition for stoichiometry.

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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. How is percent yield calculated?

Question 13 13. 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 14 14. How is a mole ratio used?

Question 15 15. What does the empirical formula show?

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

Question 18 18. 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 19 19. What is the volume of 2 moles of a gas at 300K and 1.25atm?

Question 20 20. If there are three moles of H2 O for every one mole of LiClO4, then what is the hydrate formula?

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Question 21 21. How do you determine the amount of product made?

Question 22 22.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

Question 23 23. What is NOT a step in determining the formula of a hydrate?

Question 24 24. How many moles of solute are in a 0.50 L solution of 3.0 molarity?

Question 25 25. Conservation of matter means that:

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Question 26 26. 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 27 27.

Choose the correctly balanced equation for the following reaction:

Potassium + water → potassium hydroxide + hydrogen gas

Question 28 28. What is a coefficient?

Question 29 29. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

Question 30 30. What is the empirical formula of a compound containing (by mass) 36.5% sulfur and 63.5% iron?

Physical Science - 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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