Gases Jeopardy

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GasesJeopardy
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Calculations for 100pts.

• Convert 78 C to Kelvin

351 K
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KMT for 100pts.

• What is a perfectly elastic collision?

A collision in which no energy is lost
.
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P, V, n, T for 100pts.

• Name three metric pressure units.

kPa, atm mmHg
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Theory for 100pts.

• As atmospheric pressure increases the column of
  mercury in a barometer

Increases in height.
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Calculations for 200pts.

• Convert 85.93 kPa to mmHg.

644.5 mmHg
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KMT for 200pts.

• Describe the motion of ideal gas particles.

Ideal gas particles are in constant moltion.
Ideal gas particles move in straight lines until
they collide with another object.
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P, V, n, T for 200pts.

• Define pressure.

Pressure is the force per area.
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Theory for 200pts.

• Explain the concept of molar volume.

Molar volume is the volume of one mole of gas at
STP, which is the same for all gases.
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Calculations for 300pts.

• A balloon has a volume of 11.8 L when the
  temperature is 57.0C. What would the volume of
  the balloon be if the temperature is decreased to
  25.0C, if the pressure and amount of gas are
  constant?

10.7 L
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KMT for 300pts.

• Real gas particle exert _____ forces on each
  other.

Attractive
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P, V, n, T for 300pts.

• What is standard temperature in Kelvin and
  standard pressure in kPa?

273 K and 101.325 kPa
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Theory for 300pts.

• How is the volume and the amount of gas related
  if temperature and pressure are held constant?

Volume and amount of gas are directly
proportional to each other.
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Calculations for 400pts.

• 2.5 liters of carbon dioxide are collected over
  water at 25ºC and 99.0 kPa. What is the volume of
  the gas as standard pressure, if the temperature
  remains constant?

2.4 L
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KMT for 400pts.

• Why do gases not have a fixed volume?

Gas molecules are separated by much space and can
be compressed or expanded to fill the volume of
their container.
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P, V, n, T for 400pts.

• Gay-Lussacs Law of Combining Volumes applies to
  gas reactions at

a constant temperature and pressure.
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Theory for 400pts.

• For gas sample of constant number of moles and
  pressure what is the relationship between volume
  and temperature?

Volume and temperature are directly proportional.
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Calculations for 500pts.

• A 57.0 mL of gas is collected over water at
  5.00?C and 75.0 kPa, what is the volume of the
  dry gas at STP?

40.9 mL
RETURN
RETURN
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KMT for 500pts.

• What two factors cause a gases to diffuse faster?

Small molecules and high temperature.
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P, V, n, T for 500pts.

• Define pressure.

Pressure equals force per unit area.
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Theory for 500pts.

• For gas sample of constant number of moles and
  temperature what is the relationship between
  volume and pressure?

Volume and pressure is indirectly proportional.
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Calculations for 600pts.

• How many liters of oxygen measured at STP are
  needed to burn 10.0 grams of magnesium?
• 2Mg(s) O2(g) ? 2MgO(s)

4.61 L
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KMT for 600pts.

• Name three ways to increase a gas pressure.

Increase the temperature, decrease the volume or
increase the amount of gas
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P, V, n, T for 600pts.

• Convert 4.68 L to cubic centimeters.

4680 cm3
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Theory for 600pts.

• What is the difference between effusion and
  diffusion?

Both are the movement of gas molecules. Diffusion
is when gas molecules spread out through a space,
but effusion is the movement of gas particles
through a small opening.
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Calculations for 700pts.

• How many liters of PCl5 are produced from 20.0
  grams of Cl2 at temperature of 27ºC and a
  pressure of 104 kPa?
• PCl3(g) Cl2(g) ? PCl5(g)

6.76L
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KMT for 700pts.

• What kind of gases does the Kinetic Molecular
  Theory define?

Ideal gases
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P, V, n, T for 700pts.

• Why must the partial pressure of water be
  subtracted from the measured pressure of a gas
  collected over water.

Gas collected over water is a mixture of gas and
water vapor. For further calculations for the gas
the pressure of just the gas collected must be
used.
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Theory for 700pts.

• How could the ideal gas constant, R, be derived?

PV/nT R
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Calculations for 800pts.

• What is the volume of 6.00g of chlorine at 201kPa
  and 10.5 C?

0.996 L
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KMT for 800pts.

• Explain the difference between the molecules of a
  gas and a liquid or solid.

Gas molecule have more motion and space between
them than molecules of a liquid or solid.
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P, V, n, T for 800pts.

• The pressure of a constant mass of gas is tripled
  at constant temperature, the volume of the gas is
  reduced to ___ its original size.

One third.
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Theory for 800pts.

• Give the kinetic explanation of Boyles Law as
  the volume of a sample of gas decreases.

• As the volume decreases the molecules have less
  room and collide with the contain more often
  which increases the pressure.

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Calculations for 900pts.

• What is the density of oxygen gas at standard
  temperature and pressure?

1.43 g/L
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KMTfor 900pts.

• How does a gas exert pressure on an object?

The gas molecules collide with the object.
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P, V, n, T for 900pts.

• Describe how a mercury barometer works.

Air molecules exert pressure on the surface of
the mercury. As the pressure increases this
increases the level of the mercury in the tube.
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Theory for 900pts.

• Give the kinetic explanation of Charles Law as a
  sample of gas decreases in temperature.

• As temperature decreases the particles move
  slower and collide with the container less often
  and with less force. If the container is elastic
  it will get smaller.

RETURN
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Calculations for 1000pts.

• If 15.0 liters of hydrogen are reacted with
  excess nitrogen, how many liters of ammonia are
  produced?N2 (g) 3H2 (g) ? 2NH3 (g)

10.0 L
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KMT for 1000pts.

• What is the relationship between real gas
  molecules and ideal gas molecules at common
  temperatures and pressures?

Real gases act like ideal gases at common
temperatures and pressures.
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P, V, n, T for 1000pts.

• What is the definition of temperature?

A measure of the average kinetic energy of the
particles
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Theory for 1000pts.

• Water is boiled in a soda can. The can is flipped
  upside down into cool water. The can collapses.
  Using the kinetic molecular concepts of pressure
  temperature and volume explain how this happened.

As the molecules of the water and air heat they
move faster and leave the can. When the can is
cooled quickly the molecule slow down and
condense producing a lower pressure inside the
can. The high pressure outside the can crushes
the can.
RETURN