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Which statement best describes molar mass? a. the mass of 6.02 x 10²3 atoms, which is constant for all substances b. the mass in grams of 6.02 x 1023 particles of a given substance, which is unique to each substance C. the mass of a substance that is required to be visible to the naked eye d. the mass of particles in exactly 1.0 L of gas

Which statement best describes molar mass? a. the mass of 6.02 x 10²3 atoms, which is constant for all substances b. the mass in grams of 6.02 x 1023 particles of a given substance, which is unique to each substance C. the mass of a substance that is required to be visible to the naked eye d. the mass of particles in exactly 1.0 L of gas

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1. Which statement best describes molar mass? a. the mass of 6.02 x 1023 atoms, which is constant for all substances b. the mass in grams of 6.02 x 10²3 particles of a given substance, which is unique to each substance 2. An element X has a molar mass of 40.0 g/mol. How many moles are in 10 grams of element X? a. 400 moles c. 0.250 moles d. 25.0 moles b. 4.00 moles 4. c. the mass of a substance that is required to be visible to the naked eye d. the mass of particles in exactly 1.0 L of gas 3. Which statement is true according to the Law of Definite Proportions? a. A chemical compound always contains the same proportions of elements by mass b. A chemical compound always contains the same proportions of elements by molar ratio C. A chemical compound always contains the same proportions of elements by volume d. A chemical compound can contain any proportion of elements by mass 5. What would be the molar mass of germanium tetrafluoride? a. 129.62 g/mol b. 148.63 g/mol Which of the following is not an empirical formula? a. X3Y7 b. X₂Y8Z c. 91.63 g/mol d. 110.63 g/mol 6. The Law of Multiple Proportions states that: a. Atoms can combine with each other in only one ratio to form a chemical compound b. Atoms can combine with each other in any ratio to form a chemical compound C. X₂Y2Z2 b. careful transfer of all reactants c. a foreign substance being added to the product container d. some reactant being lost to evaporation c. Atoms can combine with each other in whole number ratios to form chemical compounds d. Adding more molecules of a substance to the same substance changes the ratio of the atoms in that substance 7. Which of the following factors would not increase the calculated percent yield of a reaction? a. using higher purity reactants 8. Drivers ascending high mountain passes sometimes find that their engines suddenly stop running as they increase in altitude, even with plenty of fuel. What is the limiting reactant in their engine? a. gasoline b. heat a. 4.0 moles b. 2.0 moles c. oxygen d. none of the above 9. How many atoms are contained in 1.81 x 1024 molecules of carbon dioxide? (n = Avogadro's number) a. n b. 3n d. X₂Y8Zs c. n d. 9n 10. How many moles of lithium are produced from the decomposition of 4.0 moles of lithium oxide? C. 8.0 moles d. More information needed
Transcribed Image Text:1. Which statement best describes molar mass? a. the mass of 6.02 x 1023 atoms, which is constant for all substances b. the mass in grams of 6.02 x 10²3 particles of a given substance, which is unique to each substance 2. An element X has a molar mass of 40.0 g/mol. How many moles are in 10 grams of element X? a. 400 moles c. 0.250 moles d. 25.0 moles b. 4.00 moles 4. c. the mass of a substance that is required to be visible to the naked eye d. the mass of particles in exactly 1.0 L of gas 3. Which statement is true according to the Law of Definite Proportions? a. A chemical compound always contains the same proportions of elements by mass b. A chemical compound always contains the same proportions of elements by molar ratio C. A chemical compound always contains the same proportions of elements by volume d. A chemical compound can contain any proportion of elements by mass 5. What would be the molar mass of germanium tetrafluoride? a. 129.62 g/mol b. 148.63 g/mol Which of the following is not an empirical formula? a. X3Y7 b. X₂Y8Z c. 91.63 g/mol d. 110.63 g/mol 6. The Law of Multiple Proportions states that: a. Atoms can combine with each other in only one ratio to form a chemical compound b. Atoms can combine with each other in any ratio to form a chemical compound C. X₂Y2Z2 b. careful transfer of all reactants c. a foreign substance being added to the product container d. some reactant being lost to evaporation c. Atoms can combine with each other in whole number ratios to form chemical compounds d. Adding more molecules of a substance to the same substance changes the ratio of the atoms in that substance 7. Which of the following factors would not increase the calculated percent yield of a reaction? a. using higher purity reactants 8. Drivers ascending high mountain passes sometimes find that their engines suddenly stop running as they increase in altitude, even with plenty of fuel. What is the limiting reactant in their engine? a. gasoline b. heat a. 4.0 moles b. 2.0 moles c. oxygen d. none of the above 9. How many atoms are contained in 1.81 x 1024 molecules of carbon dioxide? (n = Avogadro's number) a. n b. 3n d. X₂Y8Zs c. n d. 9n 10. How many moles of lithium are produced from the decomposition of 4.0 moles of lithium oxide? C. 8.0 moles d. More information needed
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