Chemistry 11 December Practice Quiz
1)
Describe an example of how you can or have used the
scientific method in the lab or elsewhere in your life. Use the language of the scientific method
(observation, hypothesis, etc.) in your description.
2)
Sketch the “Map of the Physical Universe.”
3) Convert to the stated units:
a) 213 mg to kg
b) 12.11 cs to ms
c)
6.4 g/mm3 to kg/m3
4) Give the following in decimal form:
a) 8.2 × 103
b) 2.13 × 10-5
5) Give the following in scientific notation:
a) 746000
b) 0.000065
6) Calculate with correct sig figs 1.01 ×
4.0000/2.020 =
7)
What volume does 5.0 mg of acetone have?
8) Compare the macroscopic and microscopic properties of sold and liquid
phases.
9) Water ice at 0ºC is melted to make liquid water at 0ºC by adding 200,000
J of heat energy. How much ice will be
melted?
10) 500 g of liquid water at 10ºC releases 17,000 J of heat energy. What will its final temperature be?
11) Heat
a)
What does absolute zero signify?
b)
What is absolute zero in Celsius, Kelvin?
c)
What is 0oC in Kelvin?
d)
Sketch and label the temperature vs time
graph for a 1.0 kg chunk of copper in a closed container, initially at 500o
C, that is then heated steadily until it is at 3000o C.
e)
How much heat energy is needed to raise the copper to its melting
point?
f)
How much heat energy is needed to melt the copper?
12) Phases and phase change
a) How do a liquid and a gas
differ on the macroscopic and microscopic scales?
b)
Calculate how many moles of gas occupy one liter at STP.
13) Consider the graph here:
a) What is the melting point for this substance?
b) What is the boiling point for this substance?
c) For which phase is the specific heat biggest?
d) For which phase is the specific heat smallest?
14) In your own words describe what you observed in Lab #8
on Charles’ Law. (Hint: you put the
plastic bag filled with air into ice water…).
In particular, describe how the volume of gas changed as the temperature
changed.
15) A mixture of gases at 2.4 atm
total pressure is made up of equal parts of helium, oxygen and nitrogen. What is the partial pressure of each
gas? Bonus: If you doubled the amount of helium gas and kept the total pressure
the same, what would the partial pressure of each gas be?
16) A sample of helium gas of volume 1.5 L is at STP (I
will expect you to know what this means for the test). How many moles of helium are there?
17) A rigid box contains gas at 20ºC and a pressure of 1.6
atm. What will
the pressure be at 100ºC?
18) Do the following conversions:
a) 650 Torr to Pa
b) 2.26 × 1024units to moles
c) 95 mL to m3
19) Types of Atomic Matter
a)
What are the large scale properties of a homogeneous mixture?
b)
Describe an ionic compound microscopically
20) Solutions
a)
Describe how you would go about making 3.0 L of a 0.20M solution of
salt in water. Give numbers!
b)
What volume of this solution would I need to get 0.020 moles of salt?
c)
Describe the effect on boiling and melting point of adding salt to water
d)
Why do you think they salt the roads in
21) The Mole and the periodic
table
a)
What is the atomic number for tin?
b)
What is the symbol for mercury?
c)
What is the molar mass of carbon?
d)
What is the molar mass of ethane (C2H6)?
e)
How many moles of ethane are there in 10g of it?
f)
How many moles of hydrogen atoms are there in 10g of ethane?
g)
How much mass is 7.0 moles of ethane?
22) Balance and give the reaction type:
a)
Fe + CuSO4 ------> Cu + FeSO4
b)
KNO3 + Pb(OH) 2 ------> Pb(NO3) 2 + KOH
c)
C8H18 + O2 ------> CO2 + H2O
d)
H2O2 ------> H2O + O2
23) Consider reaction 22d):
a)
If 19.0 grams of H2O2 are mixed to make 2.4 liters of solution what is
the initial concentration?
b)
How many of grams of oxygen will be produced if all the H2O2 is converted?
c)
How many moles of water will be produced?
24) How would you go about
finding the density of an irregularly shaped chunk of gold colored metal? How would you use this result to see what the
metal was (assuming it is a pure substance)?
How might you confirm this result?
Data:
Density of acetone: 790
kg/ m3
Conversion factor for liters: 1000
L = 1.000 m3
Latent heat of fusion
for copper: 2.0
× 105 J/kg
Latent heat of
vaporization for copper 5.0
× 106 J/kg
Melting point for
copper: 1000oC
Boiling point for
copper: 2500oC
Specific heat capacity
for solid copper: 400
J/kg Co
Specific heat capacity
for molten (liquid) copper: 600 J/kg Co