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Mastering Chemical Quantities for Chemistry Success

Dive into chemical quantities with this review. Explore empirical formulas, molar masses, Avogadro's number, density of gases, and more.

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Mastering Chemical Quantities for Chemistry Success

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  1. Chapter 10 Review“Chemical Quantities”

  2. Chapter 10 Review • Which of the following sets of empirical formula, molar mass, and molecular formula is correct: a) CH, 78 g, C13H13, or b) CH4N, 90 g, C3H12N3? • What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?

  3. Chapter 10 Review • What SI unit is used to measure the number of representative particles in a substance? • Avogadro’s number of representative particles is equal to one ____. • The molar mass of a certain gas is 49 g. What is the density of the gas in g/L at STP?

  4. Chapter 10 Review • A 22.4 L sample of which of the following substances, at STP, would contain 6.02 x 1023 representative particles: a) oxygen, or b) gold? • Which combination of temperature and pressure correctly describes standard temperature and pressure, STP?

  5. Chapter 10 Review • Which of the following is NOT true about atomic mass: a) the atomic mass is 12 g for magnesium, or b) the atomic mass is the mass of one mole of atoms? • Which of the following elements exists as a diatomic molecule: a) lithium, or b) nitrogen?

  6. Chapter 10 Review • Which of the following gas samples would have the largest number of representative particles at STP: a) 12.0 L He, or b) 7.0 L O2? • The molar volume of any gas at STP occupies ____. • What is the molar mass of AuCl3? • The lowest whole-number ratio of the elements in a compound is called the ____.

  7. Chapter 10 Review • Given 1.00 mol of each of the following gases at STP, which gas would have the greatest volume: a) He, or b) SO3? • What is the number of moles in 500 L of He gas at STP? • What is the percent composition of chromium in BaCrO4?

  8. Chapter 10 Review • How many atoms are in 0.075 mol of titanium? • How many molecules are in 2.10 mol CO2? • How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O?

  9. Chapter 10 Review • If the density of an unknown gas “Z” is 4.50 g/L at STP, what is the molar mass of gas “Z”? • If 60.2 g of Hg combines completely with 24.0 g of Br to form a compound, what is the percent composition of Hg in the compound?

  10. Chapter 10 Review • Which of the following compounds have the same empirical formula: a) C7H14 and C10H20, or b) C6H12 and C6H14? • What is the molar mass of ammonium carbonate, (NH4)2CO3? • Know the comparisons between an empirical and molecular formula.

  11. Chapter 10 Review • What is the molar mass of chlorine gas? • The volume of one mole of a substance is 22.4 L at STP for all ____. • Which of the following is NOT an empirical formula: a) C2N2H8, or b) C3H8O?

  12. Chapter 10 Review • How many moles of tungsten atoms are in 4.8 x 1025 atoms of tungsten? • What information is needed to calculate the percent composition of a compound? • What is the density at STP of the gas sulfur hexafluoride, SF6? • Know the values that Avogadro’s number is equal to.

  13. Chapter 10 Review • How many moles of silver atoms are in 1.8 x 1020 atoms of silver? • Determine the mass in grams of 3.10 x 1023 molecules of F2. • Find the number of moles of argon in 607 g of argon. • Find the mass, in grams, of 1.40 x 1023 molecules of N2.

  14. Chapter 10 Review End of Chapter 10 Review

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