5. Faster, because if a substance or mixture is heated, the kinetic energy of the particles in the substance
6. High energy
7. The kelvin temperature of the enclosed gas doubles, the pressure of the enclosed gas also doubles and causing the container to bursts.
8. The volume of the gas is halved and the pressure doubled.
Gas Laws:
- Boyle’s Law- Pressure and Volume
a.
Pressure increases as you fill a tire with air because:
As you increase the # of gas particles the # of collisions
between particles and the walls of the container increases
b.
Reducing volume causes an increase in pressure because:
reducing the volume causes the number of
collisions with the container to increase , increasing pressure
c.
Boyle’s Law- For a given mass of gas at constant
temperature, the volume of the gas varies inversely with pressure.
a.
As one goes up ,
the other goes down .
b.
P x V = K Pressure times volume is constant provided the
temperature and amount of gas do not change.
A gas with a volume of 4.00
L at a pressure of 205 kPa is allowed to expand to a volume of 12.0 L. What is
the pressure in the container if the temperature remains constant?
P1 x V1
= P2 x P2
250
kPa x 4.00 L = P2 x 12.0 L
P2 = 250 kPa
x 4.00 L/12.0 L
P2
= 83.33 kPa
Charles’ Law- Temperature and
volume
A.
Relationship between temperature and volume can only be
studied for a limited range of temperatures because: gases condense at low temperature
B.
Charles’s Law: The volume of a fixed mass of gas is
directly proportional to its KELVIN temperature if the pressure is
constant.
1) as one variable goes up ,
the other goes up .
2)
V/T = K at
constant mass and pressure.
Exactly
5.00 L of air at -50.0oC is warmed to 100.0 oC. What is the new volume if the pressure
remains constant? V1/T1 = V2/T2
T1 = -50.0oC + 273 = 223 K
T2 = 100.0oC + 273 = 373 K 5.00 L/223 K = V2/373 K
V2 = 5.00 L/223 K x 373 K
V2 = 8.36 L
- Gay-Lussac’s
Law- Temperature and Pressure
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