HW Review
Qualtiative Analysis WS II and
Nomenclature
a)
b)
c)
d)
e)
f)
g)
h)
i)
j)
k)
l)
m)
n)
o)
p)
q)
r)
lithium chloride
magnesium hydroxide
Potassium phosphide
Iron III oxide
Iron II oxide
Zinc chloride
Silver nitrate
Ammonium chloride
Copper II chloride
Tin II chloride
Lead IV oxide
Aluminum chloride
Lead II sulfate
Magnesium phosphate
sodium carbonate
Sodium bicarbonate
Potassium cyanide
Potassium permanganate
Nomenclature 1
Nomenclature 3
a)
b)
c)
d)
e)
f)
g)
h)
i)
j)
Carbon monoxide
Carbon dioxide
Dihydrogen monoxide
Carbon tetrachloride
Dinitrogen trioxide
Silicon dioxide
Dinitrogen monoxide
Carbon tetra bromide
Sulfur dioxide
Disulfur dichloride
Quantitative Chem II
7. CH2O
10. C10H24O2
11. C4H6
14. C2H6O
Gases WS II
• 13. a) the root mean square velocity of He is
greater than that of Kr. This is due to the fact
that the molar mass of He is less than Kr. The
square root of the molar mass is in the
denominator of the equation. Smaller
denominator (MM) will yield a higher
velocity.
• B) the temperature must increase in order to
increase the avg. speed of atoms.
Diffusion
Diffusion: describes
the mixing of gases.
The rate of diffusion is
the rate of gas mixing.
Effusion
• Passage of gas through a small hole, into a
vacuum.
• The effusion rate measures how fast this
happens.
• Graham’s Law the rate of effusion is inversely
proportional to the square root of the mass of
its particles.
Rate of effusion for gas 1
M2

Rate of effusion for gas 2
M1
Graham’s Law
Rates of Effusion and Diffusion
Effusion:
Rate of effusion for gas 1

Rate of effusion for gas 2
M2
M1
Diffusion:
Distance traveled by gas 1

Distance traveled by gas 2
M2
M1
Gases WS II
14. Two factors that cause deviations are an
increase in attractive forces between particles and a
reduction in free space relative to the volume of the
container. At low T, gas particles are closer and
move slower. Forces of attraction exist between gas
particles when they are in close proximity and these
forces reduce the expected pressure excreted by
the gas.
Ideal gas law assumes that gas particles don’t have
V of their own as it is negligible compared to V of
container. When the V occupied by the particles
makes up a high percentage of total volume of the
container gas does not behave ideally.
Gases WS II
• 15
Average distance between gas particles
increases as P decreases. When particles are
further apart attractive forces between particles
are greatly reduced. This is why gas particles will
behave as they have no interaction with one
another. Therefore there is no reduction in the
expected pressure due to the forces of
attraction between particles.
Gases WS II
• 16. a) 181 atm
b) When gases are behaving ideally there are no
forces of attraction. No forces slowing them down
before they strike container. We do have forces of
attraction when they are close to one another.
These attractive forces reduce the expected
pressure of the gas. They will pull on the gas
particles and cause the reduction in force when
they hit the container and therefore reduce the
pressure.