
1 
6.37 grams of ice at 0^{o}C
occupy a volume of 6.95 mL. What is the density of ice at 0^{o}C 



1.00 g/mL 



0.917 g/mL 



1.09 g/mL 



9.165468x10^{1} g/mL 



None of the previous answers. 

2 
2.50 mL of mercury weighs 34.0 grams
at 20^{o}C. What is the density of mercury at 20^{o}C? 



7.35x10^{2} g/mL 



85.0 g/mL 



13.6 g/mL 



14 g/mL 



None of the previous answers. 

3 
A cylinder of manganese (length 4.00
cm, diameter = 1.00 cm) has a mass of 22.62 g. What is the density of manganese? 



1.80 g/cm^{3} 



5.66 g/cm^{3} 



0.139 g/cm^{3} 



7.20 g/cm^{3} 



None of the previous answers. 

4 
An irregular 77.7 g piece of silver
is placed into a graduated cylinder that has 15.0 mL of water in it. The new water level
is 22.4 mL. What is the density of the silver? 



1.0x10^{1} g/cm^{3} 



10.5 g/cm^{3} 



0.095 g/cm^{3} 



3.5 g/cm^{3} 



None of the previous answers. 

5 
26% by mass aqueous sodium chloride
is added to a graduate cylinder (mass of cylinder = 85.550 g) to the 35.0 mL mark. The
cylinder and contents now weigh 127.445 g. What is the density of the sodium chloride
solution? 



1.00 g/mL 



3.64 g/mL 



0.835 g/mL 



1.197 g/mL 



None of the previous answers. 

6 
The density of 100% sulfuric acid is
1.83 g/mL. How many mL do you need to provide 75.0 g of sulfuric acid? 



137 mL 



0.0244 mL 



41.0 mL 



75.0 mL 



None of the previous answers. 

7 
The density of oxygen gas at 1
atmosphere pressure and 25^{o}C is 1.31 g/L. How many mL do you need of oxygen gas
to provide 5.00 g of oxygen gas? 



3.82x10^{3} mL 



3.82 mL 



6.55x10^{3} mL 



262 mL 



None of the previous answers. 

8 
Bromine is the only nonmetal that
exists as a liquid at room temperature. This dangerous and very toxic substance has a
density of 3.12 g/mL. What is the mass of 25.0 mL of bromine? 



8.01 g 



78.0 g 



0.125 g 



78 g 



None of the previous answers. 

9 
A spherical container with a
diameter of 26.0 cm contains 10.6 g of nitrogen at 1 atmosphere pressure and 25^{o}C.
What is the density of the nitrogen gas? 



0.144 g/L 



1.15x10^{3} g/L 



0.868 g/L 



1.15 g/L 



None of the previous answers. 

10 
Very approximately, the density of
gases is how many times less than the density of liquids? 



0.001 



1000 



10 



100 



None of the previous answers. 

11 
If the density of gasoline is 0.70
g/mL, what is the mass in grams of 1.4x10^{1} L of gasoline? 



9.8x10^{2} g 



98 g 



5x10^{3} g 



2x10^{4} g 



None of the previous answers. 

12 
270 mL of water has a mass of about: 



2.7 g 



2.70x10^{2} g 



2.7x10^{5} g 



2.7x10^{4} g 



None of the previous answers. 

13 
The density of copper is 8.92 g/mL.
The volume of a piece of copper that has a mass of 10.0 g is: 



0.892 mL 



1.12 mL 



89.2 mL 



10.0 mL 



None of the previous answers. 

14 
The story of Air Canada Flight 143
(made into a movie as Flight 171) from Montreal to Edmonton on 7/23/83, affords an
interesting and relevant example of the importance of unit conversions (P. Banks, Chem.
Matters, 10/96, 1215). A ground crew determied that the flight would require 22,300
kg of fuel for the flight and the tanks contained 7,682 Liters. To calculate how many
liters of fuel needed to be added, they used a conversion factor of 1.77 and assumed the
units were kg/L. Unfortunately the conversion factor 1.77 has units of lbs/L. From 1.77
lbs/L, calculate the conversion factor in kg/L. For a map of Canada, see:
http://members.tripod.com/policecars1/canadamap.htm.




3.90 kg/L 



1.24 kg/L 



0.803 kg/L 



None of the previous answers. 





15 
Every time a problem is solved, you
should ask if the conversion factors used and the answer make sense. The ground crew
assumed the density of the fuel to be 1.77 kg/L. Consider the density of water and of fuel
(are fuels such as gasoline more or less dense than water?). The factor 1.77 kg/L doesn't
make sense and the ground crew should have but did not catch their own mistake and loaded
the plane with the amount of fuel based on 1.77 kg/L. Calculate the volumes in liters
needed respectively using the incorrect 1.77 kg/L and the correct value. 



4.92x10^{3} L, 2.01x10^{4 L} 



1.54x10^{4} L, 1.30x10^{4 L} 



None of the previous answers. 









16 
Calculate the shortage in liters of
gasoline that resulted from the use of 1.77 kg/L instead of the correct value.
(Incidentally, thanks to the heroic work of the flight crew and the air controllers, the
flight made a safe emergency landing on an abandoned air strip near Winnipeg considerably
short of its destination. In this case a tragedy was averted by both a careful response to
the problem and luck. However, proper use of conversion factors with appropritate units
coupled with some thinking would have avoided the need for the heroics and a chance for
tragedy.) For more information on Flight 143, see: http://en.wikipedia.org/wiki/Gimli_Glider
http://archives.cbc.ca/on_this_day/07/23/
http://hawaii.hawaii.edu/math/Courses/Math100/Chapter1/Extra/CanFlt143.htm 



more fuel than needed 



1.52x10^{4} L 



None of the previous answers. 








