chapter 10 chemistry

Which combination of temperature and pressure correctly describes standard temperature and pressure, STP? a. 0 C and 101 kPa c. 0 C and 22.4 kPa b. 1 C and 0 kPa d. 100 C and 100 kPa

0 degrees C and 101 kPa

What is the number of moles in 9.63 L of H2S gas at STP? a. 0.104 mol c. 3.54 mol b. 0.430 mol d. 14.7 mol

0.430 mol

How many molecules are in 2.10 mol CO2? a. 2.53 x 10^24 molecules c. 3.49 x 10^24 molecules b. 3.79 x 10^1 molecules d. 1.26 x 10^24 molecules

1.26 x 10^24 molecules

What is the number of moles in 432 g of Ba(NO3)2? a. 0.237 mol c. 1.65 mol b. 0.605 mol d. 3.66 mol

1.65 mol

Butanol is composed of carbon, hydrogen, and oxygen. If 1.0 mol of butanol contains 6.0 x 10²⁴ atoms of hydrogen, what is the subscript for the hydrogen atom in C₄H₂O? a. 1 c. 6 b. 10 d. 8

10

What is the volume, in liters, of 0.500 mol of C3H8 gas at STP? a. 0.0335 L c. 16.8 L b. 11.2 L d. 22.4 L

11.2 L

Which of the following gas samples would have the largest number of representative particles at STP? a. 12.0 L He c. 0.10 L Xe b. 7.0 L O d. 0.007 L SO3

12.0 L He

What is the mass of oxygen in 250 grams of sulfuric acid, H2SO4? a. 0.65 g c. 16 g b. 3.9 g d. 160 g

160 g

How many atoms are in 3.5 moles of arsenic atoms? a. 5.8 x 10 atoms c. 2.1 x 10 atoms b. 7.5 x 10 atoms d. 1.7 x 10 atoms

2.1 x 10^24

What is the mass of silver in 3.4 g AgNO3? a. 0.025 g c. 2.2 g b. 0.64 g d. 3.0 g

2.2 g

The molar mass of a certain gas is 49 g. What is the density of the gas in g/L at STP? a. 3.6 10 g/L c. 2.2 g/L b. 0.46 g/L d. 71 g/L

2.2 g/L

How many moles of CaBr2 are in 5.0 grams of CaBr2? a. 2.5 x 10^-2 mol c. 4.0 x 10^2 mol b. 4.2 x 10^-2 mol d. 1.0 x 10 mol

2.5 x 10^-2 mol

What is the percent composition of chromium in BaCrO4? a. 4.87% c. 20.5% b. 9.47% d. 25.2%

20.5%

What is the number of moles in 500 L of He gas at STP? a. 0.05 mol c. 22 mol b. 0.2 mol d. 90 mol

22 mol

The molar volume of a gas at STP occupies _______. a. 22.4 L c. 1 kilopascal b. 0 C d. 12 grams

22.4 L

Which expression represents the percent by mass of nitrogen in NH4NO3 a. 14 g N/80 g NH4NO3 x 100% b. 28 g N/80 g NH4NO3 x 100% c. 80 g NH4NO3 /14 g N x 100% d. 80 g NH4NO3 /28 g N x 100%

28 g N/80 g NH4NO3 x 100%

How many moles of silver atoms are in 1.8 x 10^20 atoms of silver? a. 3.0 x 10^-4 c. 3.0 x 10^4 b. 3.3 x 10^-3 d. 1.1 x 10^44

3.0 x 10^-4

What is the molar mass of AuCl3? a. 96 g c. 232.5 g b. 130 g d. 303.6 g

303.6 grams

How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O a. 5 (6.02 10 ) c. 35 b. 5 d. 35 (6.02 10 )

35

What is the number of moles of beryllium atoms in 36 g of Be? a. 0.25 mol c. 45.0 mol b. 4.0 mol d. 320 mol

4.0 mol

How many atoms are in 0.075 mol of titanium? a. 1.2 x 10^-25 c. 6.4 x 10^2 b. 2.2 x 10^24 d. 4.5 x 10^22

4.5 x 10^22

If the density of an unknown gas Z is 4.50 g/L at STP, what is the molar mass of gas Z? a. 0.201 g/mol c. 26.9 g/mol b. 5.00 g/mol d. 101 g/mol

5.00 g/mol

If 20.0 grams of Ca combines completely with 16.0 grams of S to form a compound, what is the percent composition of Ca in the compound? a. 1.25% c. 44.4% b. 20.0% d. 55.6%

55.6%

What is the density at STP of the gas sulfur hexafluoride, SF6? a. 0.153 g/L c. 3270 g/L b. 6.52 g/L d. 3.93 x 10^49 g/L

6.52 g/L

What is the percent by mass of carbon in acetone, C3H6O? a. 20.7% c. 1.61% b. 62.1% d. 30.0%

62.1%

What is the mass in grams of 5.90 mol C8H18? a. 0.0512 g c. 389 g b. 19.4 g d. 673 g

673 g

If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a compound, what is the percent composition of Hg in the compound? a. 28.5% c. 71.5% b. 39.9% d. 60.1%

71.5%

How many moles of tungsten atoms are in 4.8 x 10^25 atoms of tungsten? a. 8.0 x 10^2 moles c. 1.3 x 10^-1 moles b. 8.0 x 10^1 moles d. 1.3 x 10^-2 moles

8.0 x 10^1 moles

What is the percent composition of carbon, in heptane, C7H16? a. 12% c. 68% b. 19% d. 84%

84%

What is the molar mass of (NH4)2CO3? a. 144 g c. 96 g b. 138 g d. 78 g

96 g

Given 1.00 mole of each of the following gases at STP, which gas would have the greatest volume? a. He c. SO b. O d. All would have the same volume.

All would have the same volume

If the density of a noble gas is 1.783g/L at STP, that gas is _________. a. Kr c. Ar b. Xe d. He

Ar

Which of the following compounds has the lowest percent gold content by weight? a. AuOH c. AuCl3 b. Au(OH)3 d. AuI3

AuI3

The ratio of carbon atoms to hydrogen atoms to oxygen atoms in a molecule of dicyclohexyl maleate is 4 to 6 to 1. What is the molecular formula if its molar mass is 280g? a. C4H6O1 c. C12H18O3 b. C8H12O2 d. C16H24O4

C16H24O4

What is the empirical formula of a substance that is 53.5% C, 15.5% H and 31.1% N by weight? a. C3HN2 c. C2H8N b. C4H14N2 d. CH4N7

C2H8N

Which of the following is NOT an empirical formula? a. C2N2H8 c. BeCr2O7 b. C3H8O d. Sb2S3

C2N2H8

Which of the following compounds have the same empirical formula? a. CO2 and SO2 c. C4H10 and C10H4 b. C7H14 and C10H20 d. C6H12 and C6H14

C7H14 and C10H20

Which of the following sets of empirical formula, molar mass, and molecular formula is correct? a. CH, 78 g, C13H13 c. CaO, 56 g, Ca2O2 b. CH4N, 90 g, C3H12N3 d. C3H8O, 120 g, C3H8O2

CH₄N, 90 g, C₃H₁₂N₃

Which of the following compounds has the highest oxygen content by weight? a. Na2O c. BaO b. CO2 d. H2O

H2O

What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight? a. SO c. SO3 b. SO2 d. S6O4

SO3

Which of the following is NOT a true about atomic mass? a. The atomic mass is 12 g for magnesium. b. The atomic mass is the mass of one mole of atoms. c. The atomic mass is found by checking the periodic table. d. The atomic mass is the number of grams of an element that is numerically equal to the mass in amu.

The atomic mass is 12 g for magnesium

Which of the following is NOT true about empirical and molecular formulas? a. The molecular formula of a compound can be the same as its empirical formula. b. The molecular formula of a compound can be some whole-number multiple of its empirical formula. c. Several compounds can have the same empirical formula, but have different molecular formulas. d. The empirical formula of a compound can be triple its molecular formula.

The empirical formula of a compound can be triple its molecular formula.

What information is needed to calculate the percent composition of a compound? a. the weight of the sample to be analyzed and its density b. the weight of the sample to be analyzed and its molar volume c. the formula of the compound and the atomic mass of its elements d. the formula of the compound and its density

The formula of the compound and the atomic mass of its elements

What is true about the molar mass of chlorine gas? a. The molar mass is 35.5 g. b. The molar mass is 71.0 g. c. The molar mass is equal to the mass of one mole of chlorine atoms. d. none of the above

The molar mass is 71.0 grams

Which of the following is NOT a representative particle? a. atom c. anion b. cation d. all of the above

atom

The atomic masses of any two elements contain the same number of ____. a. atoms c. ions b. grams d. milliliters

atoms

The lowest whole-number ratio of the elements in a compound is called the _______. a. empirical formula c. binary formula b. molecular formula d. representative formula

empirical formula

The molar mass of a substance can be calculated from its density alone, if that substance is a(n)____. a. element c. liquid b. gas at STP d. solid

gas at STP

The volume of one mole of a substance is 22.4 L at STP for all _______________. a. gases c. solids b. liquids d. compounds

gases

The molar mass of C7H16 and the molar mass of CaCo3 contain approximately the same number of________________. a. carbon atoms c. cations b. anions d. grams

grams

For which of the following conversions does the value of the conversion factor depend upon the formula of the substance? a. volume of gas (STP) to moles b. density of gas (STP) to molar mass c. mass of any substance to moles d. moles of any substance to number of particles

mass of any substance to mole

The mass of a mole of NaCl is the ____. a. molar mass c. molecular mass b. atomic mass d. gram atomic mass

molar mass

Avogadro's number of representative particles is equal to one ____. a. kilogram c. kelvin b. gram d. mole

mole

What SI unit is used to measure the number of representative particles in a substance? a. kilogram c. kelvin b. ampere d. mole

mole

Which of the following elements exists as a diatomic molecule? a. neon c. nitrogen b. lithium d. sulfur

nitrogen

A 22.4-L sample of which of the following substances, at STP, would contain 6.02 x 10^23 representative particles? a. oxygen c. cesium iodide b. gold d. sulfur

oxygen

To determine the formula of a new substance, one of the first steps is to find the __________. a. molar mass c. volume at STP b. percent composition d. number of particles per mole

percent composition

The molar mass of a gas can be determined from which of the following? a. the density of the gas at STP c. Avogadro's number b. the volume of a mole of the gas d. none of the above

the density of the gas at STP

All of the following are equal to Avogadro's number EXCEPT ____. a. the number of atoms of bromine in 1 mol Br b. the number of atoms of gold in 1 mol Au c. the number of molecules of nitrogen in 1 mol N d. the number of molecules of carbon monoxide in 1 mol CO

the number of atoms of bromine in 1 mol of Br₂