Holt McDougal Modern Chemistry Chapter 9: Stoichiometry Chapter Exam

Exam Instructions:

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Question 1 1. The starting point of a stoichiometric problem is _____.

Question 2 2. What is a limiting reactant?

Question 3 3. Which of the following mole ratio is NOT appropriate to the equation 6CO2+ 6H2 O = C6 H12 O6+ 6O2?

Question 4 4. 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 5 5. How do you determine the amount of product made?

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Question 6 6. 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 7 7. How many moles of Na are needed to produce 15 moles of NaCl in the reaction 2Na + Cl2 = 2NaCl?

Question 8 8. 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?

Question 9 9. Where do you look to find the molar ratio?

Question 10 10. What is theoretical yield?

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Question 11 11. At STP, how much space (in liters) will 0.750 moles of argon gas occupy?

Question 12 12. What is meant by the term molar volume?

Question 13 13. 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 14 14. 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 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 is percent yield calculated?

Question 17 17. How many moles of N2 are needed to produce 18 moles NH3 in the reaction N2 + 3H2 = 2NH3?

Question 18 18. How is a mole ratio used?

Question 19 19. Given a balanced equation involving A and B, which set of conversions must you make to change mass A to mass B?

Question 20 20. Determine the actual yield if the theoretical yield is 12 g and the percentage yield is 90%.

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Question 21 21. Select the most suitable definition for stoichiometry.

Question 22 22. Determine the percent yield if the theoretical yield is 20 g and the actual yield is 15 g.

Question 23 23. How is mass of a substance connected to its amount in mole(s)?

Question 24 24. What is the actual yield?

Question 25 25. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

Holt McDougal Modern Chemistry Chapter 9: 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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