Chemistry 1111
Exam 2
Name _______________________________________
Aqueous solution
Avogadro’s number
Boyle’s law
Charles’ law
Chemical equation
Coefficients
Concentrated solution
Concentration
Dalton’s law
Dilute solution
Henry’s law
Mass number
Molar mass
Molarity
Mole
Mole fraction
Molecular mass
Osmosis
Partial pressure
Precipitate
Saturated solution
Solubility
Solute
Solution
Solvent
Standard molar volume
Stanislov’s law
STP
Supersaturated solution
Universal (Ideal) gas law
For each definition, select the BEST term from the above list. No term is used more than once (2
pts each)
1. ______________________________________ Moles of solute per liter of solution.
2. ______________________________________ Ptotal = P1 + P2 + P3 + …
3. ______________________________________ The pressure contributed to the total pressure
by an individual gas in a mixture of gases.
4. ______________________________________ 273 K and 1atm.
5. ______________________________________ The substance that dissolves when making a
uniform mixture.
6. ______________________________________ A uniform mixture of particles.
7. ______________________________________ PV = nRT
8. ______________________________________ A solid that forms when two solutions are
mixed together.
9. ______________________________________ In a uniform mixture, the substance that does
the dissolving.
10. ______________________________________ Expresses the maximum grams of solute in
100 grams of solvent.
11. ______________________________________ A uniform mixture where the solute to
solvent ratio is small.
12. ______________________________________ The ratio of the quantity of solute to some
given unit of the solution.
When applicable, show ALL work for the following problems. Answers arrived at with NO
work shown will receive no credit.
13. A gas with a volume of 5.28 L, a pressure of 745 mm Hg and a temperature of 25.0 ºC is
expanded to a volume of 7.75 L with a pressure of 645 mm Hg. What is the final temperature
of the gas?
14. A solution is made by placing 49.3 g of KBr in water to a final volume of 215 mL of water.
a. Express this volume in liters.
b. KBr has a molecular weight of 119 g/mol. How many moles is 49.3 g KBr?
c. Calculate the molarity of the solution.
d. How many moles of KBr are present in 50.0 mL of this solution?
e. 15.0 mL of this solution is taken and water is added to a final volume of 75.0 mL. Calculate
the molarity of this diluted solution.
15. The following questions deal with the following reaction:
2NaBH4(s) + 2HCl(aq)  B2H6(g) + 2NaCl(aq) + H2(g)
a. We are reacting 0.0375 moles of NaBH4. How many moles of H2 would this amount of
NaBH4 produce?
b. What volume of H2 gas is this at 20oC and .90 atm?
c. What volume of B2H6 would this produce under the same conditions?
d. The HCl solution used in this reaction is 0.137 M. How many milliliters of HCl are needed
to react with the 0.0375 mole of NaBH4?
16. Predict the product(s) for each of the following reactions. For each reaction circle AB (for
acid-base), OR (for oxidation reduction), P (for precipitation), or NR (for no reaction). For
precipitation reactions underline the insoluble product, for oxidation-reduction circle what
is being oxidized. You do not have to balance the equations to receive credit.
a. HNO3(aq) + KOH(aq) 
AB
OR
P
NR
P
NR
P
NR
b. MgCO3(aq) + HCl(aq) 
AB
OR
c. K(s) + HBr(aq) 
AB
OR
d. BaCl2(aq) + Na2SO4(aq) 
AB
OR
P
NR
P
NR
P
NR
e. Ca(s) + NiCl2(aq) 
AB
f.
OR
KF(s) + Cl2(g) 
AB
OR
17. 42.5 L of O2 is trapped at -15oC and 720 Torr. What is the pressure, in Torr, if the volume is
compressed to 38.5L and the temperature is 80oC?
18. For a gas, what happens to:
i.
the pressure, if temperature is decreased?
ii. the volume, if pressure is increased?
iii. the volume, if moles of gas are added?
d)
What is STP in gas laws? (Name it and define the conditions).
The partial pressure of O2 required for some species to live is 130 Torr. What is the partial
pressure of O2 in the a (fraction of O2 in dry air is 0.20) jungle atmosphere (PH20 = 95 Torr),
pressure is 720 Torr.