Name: __________________________  Date: _____________

1.	The balanced equation P4(s) + 6H2(g)  4PH3(g) tells us that 5.0 mol H2	
A)	reacts with 2.5 mol P4	
B)	produces 10.0 mol PH3	
C)	cannot react with phosphorus	
D)	produces 3.3 mol PH3	

2.	How many molecules of carbon dioxide will be formed if 8.40 g of propane is burned in the following reaction?

A)	1.52 ´ 1025 molecules	
B)	1.15 ´ 1023 molecules	
C)	4.59 ´ 1023 molecules	
D)	3.44 ´ 1023 molecules	

3.	When 20.0 g C2H6 and 60.0 g O2 react to form CO2 and H2O, how many grams of water are formed?	
A)	18.0 g	
B)	58.0 g	
C)	20.0 g	
D)	none of these	

4.	Nitric acid, HNO3, contains what percent hydrogen by mass?	
A)	20.0 %	
B)	10.0 %	
C)	4.50 %	
D)	1.60 %	

5.	Adipic acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula?	
A)	C3H5O2	
B)	C3H3O4	
C)	C2HO3	
D)	C2H5O4	

6.	Vitamin C contains the elements C, H, and O. It is known to contain 40.9% C and 4.58% H by mass. The molar mass of vitamin C has been found to be about 180. The molecular formula for vitamin C is:	
A)	C2H3O2	
B)	C3H4O3	
C)	C4H6O4	
D)	C6H8O6	

7.	A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.55 L.	
A)	300 K	
B)	289 K	
C)	21.2 K	
D)	295 K	

8.	A sample of oxygen gas has a volume of 4.45 L at 27°C and 800.0 torr. How many oxygen molecules does it contain	
A)	1.15 ´ 1023 	
B)	8.71 ´ 1025 	
C)	1.27 ´ 1024 	
D)	3.16 ´ 1024 	

9.	A 4.37 gram sample of a certain diatomic gas occupies a volume of 3.00-L at 1.00 atm and a temperature of 45°C.  Identify this gas.	
A)	F2	
B)	N2	
C)	H2	
D)	O2	

10.	You are holding four identical balloons each containing 10.0 g of a different gas.  The balloon containing which gas is the largest balloon?	
A)	H2	
B)	He	
C)	Ne	
D)	All have the same volume.	

11.	Which of the following statements is true about the kinetic molecular theory?	
A)	The volume of a gas particle is considered to be small: about 0.10 mL.	
B)	Pressure is due to the collisions of the gas particles with the walls of the container.	
C)	Gas particles repel each other but do not attract one another.	
D)	Adding an ideal gas to a closed container will cause an increase in temperature.	

12.	Which conditions of P and T are most ideal for a gas?	
A)	high P, high T	
B)	high P, low T	
C)	low P, high T	
D)	low P, low T	

13.	The specific heat capacity of silver is 0.24 J/goC. How many joules of energy are needed to warm 0.881 g of silver from 25.0oC to 27.5oC?	
A)	5.8 J	
B)	0.53 J	
C)	11.1 J	
D)	9.2 J	

14.	A 59.2-g sample of aluminum at 95.0oC is dropped into 35.0 g of water at 40.0oC. What is the final temperature of the mixture? (specific heat capacity of aluminum = 0.89 J/goC; specific heat capacity of water = 4.184 J/goC)	
A)	55oC	
B)	–4.3oC	
C)	116oC	
D)	22oC	

15.	Which of the following processes is endothermic?	
A)	water droplets condensing on a soda can on a hot summer day	
B)	an ice pack getting cold (due to ammonium nitrate dissolving in water inside the pack)	
C)	thermite reaction between iron(III) oxide and aluminum (spectacular flames are observed)	
D)	freezing water to make ice cubes	

16.	Which of the following processes is exothermic?	
A)	rolling a ball up a hill	
B)	boiling water in a beaker to make steam	
C)	allowing meat to thaw after taking it out of the freezer	
D)	reacting hydrogen and oxygen gases to make water	

17.	Two metals of equal mass with different heat capacities are subjected to the same amount of heat. Which undergoes the smallest change in temperature?	
A)	The metal with the higher heat capacity.	
B)	The metal with the lower heat capacity.	
C)	Both undergo the same change in temperature.	
D)	You need to know which metals you have.	

18.	As water freezes the energy in the reaction is	
A)	released	
B)	Absorbed	
C)	neither	
D)	does not change	

19.	How much energy is absorbed when 10g ice at 0oC is heated to 75oC?	
A)	6475j	
B)	25738j	
C)	5432j	
D)	3340j	

20.	In soda pop, CO2(g) is a ______________, and water is the ______________.	
A)	solute; solvent	
B)	solvent; solute	
C)	solution; solute	
D)	solute; solution	

21.	When a solvent has dissolved all the solute it can at a particular temperature, it is said to be	
A)	diluted	
B)	unsaturated	
C)	supersaturated	
D)	saturated	

22.	Determine the concentration of a solution made by dissolving 12.7 g of sodium chloride in 750.0 mL of solution.	
A)	0.163 M	
B)	16.9 M	
C)	0.217 M	
D)	0.290 M	

23.	You have 25.00 mL of a 0.1000 M sugar solution. How much water must be added to make a 0.01159 M solution?	
A)	215.7 mL	
B)	2.90 mL	
C)	22.1 mL	
D)	190.7 mL	

24.	What is the minimum volume of a 3.95 M NaOH solution needed to make 150.0 mL of a 0.800 M NaOH solution?	
A)	15.2 mL	
B)	42.4 mL	
C)	120. mL	
D)	30.4 mL	

25.	How many grams of CaCl2 (molar mass = 111.0 g/mol) are needed to prepare 5.74 L of 0.500 M CaCl2 solution?	
A)	331 g	
B)	319 g	
C)	344 g	
D)	442 g	

26.	The total mass of a solution is 151.7 g. The solvent mass is 125.2 g. What is the mass percent of the solute?	
A)	82.5 %	
B)	28.5 %	
C)	17.5 %	
D)	11.7 %	

Answer Key

1.	D	
2.	D	
3.	D	
4.	D	
5.	A	
6.	D	
7.	B	
8.	A	
9.	A	
10.	A	
11.	B	
12.	C	
13.	B	
14.	A	
15.	B	
16.	D	
17.	A	
18.	A	
19.	A	
20.	A	
21.	D	
22.	D	
23.	D	
24.	D	
25.	B	
26.	C