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MTLE Chemistry: Stoichiometry & 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.

A piece of copper wire contains 5 moles of copper atoms. What is its mass?

(The molecular mass of copper is 63.5 g/mol.)

Question 2 2. 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 3 3. What is the percent composition of H₂SO₃?

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

Question 5 5. What is a limiting reactant?

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Question 6 6. What is meant by the term molar volume?

Question 7 7. 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 8 8. What is the difference between a hydrate and an anhydrate?

Question 9 9. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

Question 10 10. At STP, how much space (in liters) will 0.750 moles of argon gas occupy?

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Question 11 11. 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 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.

Choose the correctly balanced equation for the following reaction:

Sodium + water → sodium hydroxide + hydrogen gas

Question 14 14. How many moles of N2 are needed to produce 18 moles NH3 in the reaction N2 + 3H2 → 2NH3?

Question 15 15. How many moles of solute are in a 0.50 L solution of 3.0 molarity?

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Question 16 16. How do you determine the amount of product made?

Question 17 17.

A piece of aluminum foil has a mass of 27 grams. About how many atoms does this contain?

(Aluminum has a molecular mass of 27 g/mol.)

Question 18 18. What is the percent composition of Cu₂S?

Question 19 19. How many moles of Na are needed to produce 15 moles of NaCl in the reaction 2Na + Cl2 → 2NaCl?

Question 20 20. If 1.605 kg of mercury are used in the reaction 2Hg + O2 --> 2HgO, what is the mass of HgO, in kilograms, that are produced?

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Question 21 21. A tenth of a mole of pennies contains how many pennies?

Question 22 22. What is the empirical formula of a compound containing (by mass) 36.5% sulfur and 63.5% iron?

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

Question 24 24. What is NOT a step in determining the formula of a hydrate?

Question 25 25. 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 26 26.

Choose the correctly balanced equation for the following reaction:

Potassium + water → potassium hydroxide + hydrogen gas

Question 27 27. What does the empirical formula show?

Question 28 28. How is percent yield calculated?

Question 29 29. What is the hydrate formula when there are 0.02 moles BaCl2 and 0.04 moles H2 O?

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

MTLE Chemistry: Stoichiometry & 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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