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Section 4: Empirical and Molecular Formulas

Empirical and Molecular Formulas

1.
What relationship is described by the formula below? (mass of the element/mass of the compound) x 100
A)percent composition
B)mole ratio
C)Avogadro’s number
D)empirical formula
2.
What is the percent composition of carbon dioxide CO2?
A)73% C and 27% O
B)27% C and 73% O
C)33% C and 66% O
D)50% C and 50% O
3.
How can the actual molecular formula be determined?
A)from the empirical formula alone
B)from the molar mass alone
C)from the molar mass divided by the mass of the empirical formula
D)from the molar mass multiplied by the mass of the empirical formula
4.
An empirical formula mass is found to be 17 g/mol. The molar mass is found to be 34 g/mol. What is the number of empirical formula units in this molar mass?
A)2 units
B)0.5 unit
C)17 units
D)1 unit
5.
Analysis of a covalent compound showed that it contained 14.4% hydrogen and 85.6% carbon by mass. What is the empirical formula for this compound?
A)CH
B)CH2
C)CH3
D)C2H3
6.
A compound contains sulfur, oxygen, and chlorine. Analysis of a sample showed that it contained by mass 26.95% sulfur and 59.61% chlorine. What is the simplest formula for this compound?
A)SOCl
B)SOCl2
C)SO2Cl2
D)SO2Cl
7.
A 4.628-g sample of an iron oxide was found to contain 3.348 g of iron and 1.280 g of oxygen. What is the simplest formula for this compound?
A)FeO
B)Fe2O3
C)Fe3O4
D)FeO2
8.
What mass of iron is contained in 62.8 grams of pyrite FeS2?
A)40.3 g
B)29.2 g
C)31.7 g
D)58.5 g
9.
What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?
A)0.05 kg
B)0.2 kg
C)0.4 kg
D)0.5 kg
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