1 / 14

Chapter 10 Review “Chemical Quantities”

Chapter 10 Review “Chemical Quantities”. Chapter 10 Review. Which of the following sets of empirical formula, molar mass, and molecular formula is correct: a) CH, 78 g, C 13 H 13 , or b) CH 4 N, 90 g, C 3 H 12 N 3 ?

mchristina
Télécharger la présentation

Chapter 10 Review “Chemical Quantities”

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related