Honors Chemistry Chapter 7 Lesson 3 Quiz

What is the percentage of iron in iron(III) chloride, FeCl₃? The molar mass of FeCl₃ is 162.2 g/mol. a.) 25.00% b.) 34.43% c.) 61.17% d.) 65.57%

34.43%

One mole of potassium atoms has a mass of a.) 1g b.) 39.10 g c.) 78.20 g d.) 6.022 x 10₂₃ g

39.10 g

What is the correct molar mass of Ag₃PO₄? a.) 481.58 g/mol b.) 387.61 g/mol c.) 154.84 g/mol d.) 52.32 g/mol

418.58 g/mol

How many total moles of atoms are there in one mole of silver(I) phosphate, Ag₃PO₄? a.) 3 b.) 7 c.) 8 d.) 11

8

What is the correct formula mass for zinc hydroxide, Zn(OH)₂? a.) 83.41 g b.) 99.41 g c.) 83.41 amu d.) 99.41 amu

99.41 amu

For any molecule, formula unit, or ion, the sum of the average atomic masses of all the atoms represented in a formula is the a.) formula mass b.) ionic mass c.) molecular mass d.) atomic mass

Formula mass

A compound's molar mass is numerically equal to a.) the total number of atoms in the molecule b.) the total number of moles of the compound. c.) its mass number d.) its formula mass

Its formula mass

The mass of a molecule is found by a.) adding the masses of all the atoms in the moleule b.) dividing the total mass of all the atoms in the molecule by 6.022 x 10²³ c.) multiplying the total mass of all the atoms in the molecule by 6.022 x 10²³ d.) dividing the total mass of all the atoms in the molecule by the total number of atoms

Adding the masses of all the atoms in the molecule

Which statement shows how to correctly convert from the mass of a compound in grams to the amount of that compound in moles? a.) molar mass (g/mol) x 1/mass (g) = amount (moles) b.) molar mass (g/mol) x 6.022 x 10²³ = amount (moles) c.) mass (grams0 x 1/molar mass (g/mol) = amount (moles) d.) mass (grams) x molar mass (g/mol) = amount (moles)

Mass (grams0 x 1/molar mass (g/mol) = amount (moles)

The percentage composition of a compound is a.) the percentage by volume of each element in the compound b.) the percentage by mass of each element in the compound c.) the molar mass of the compound / the mass of each element in 1 mol of the compound d.) the mass of each element in 1 mol of the compound x the molar mass of the compound

The percentage by mass of each element in the compound