Chapter 10 Review Name
__________________________________

Period
_______ Date______________________

Classify
each of these statements as always true, AT, sometimes true, ST, or never true,
NT.

_____ 1. A mole of
a pure substance contains 6.02 x 10^{23} atoms.

_____ 2. The
representative particle of a compound is a molecule.

_____ 3. A mole of CCl_{4} is composed of one mole of carbon
and 4 mole of chlorine.

_____ 4. One mole
of gas occupies 22.4 L

_____ 5. The formula of methane is CH_{4}. If methane contains 75% carbon, then 100
grams of methane contains 75 grams of carbon.

_____ 6. The
formula for methane, CH_{4} , is both an empirical and molecular
formula.

_____ 7. The empirical formula of_{ } C_{6}H_{12}O_{6}
is C_{2}H_{4}O_{2}.

Solve
the following problems. Show your work and include the units

8. How many moles is
9.3 x 10^{15} atoms of Pb?

9.
How many representative particles are in 2.73 x 10^{-2} moles of MgI?

10.
What is the molar mass of C_{2}H_{6}?

11.
Find the mass of each of the following

A. 3.65 x 10^{-2} mol K_{2}SO_{4}

B. 2.61x 10^{22} molecules H_{2}O_{2}

C. 0.60 mol CH_{4}

D. 0.70 L Kr a STP

12.
What is the density of N_{2}O gas at STP?

13.
You have 3.8 grams of CO_{2}.
Convert that to:

A. Moles

B. Molecules

C. Atoms

D. Liters at STP

E. Find the density

14.
Determine the percent composition of CaSO_{4}.

15.
How many grams of calcium would there be in 25.3 g of CaSO_{4}
?

16.
A compound is 43.2 % copper, 24.1 % chlorine and 32.7% oxygen. What is its
empirical formula?

17. A gas is found to contain 78.1 % B and 21.9% H. It has a density of 1.23 g/L at STP. What is its

a.
empirical formula?

b.
molar mass?

c.
molecular formula?