Question

Consider a container of oxygen gas at 1 atm and 300 K. What fraction of the O2 molecules has a speed between 99% and 101% of v_rms?

Answer #1

1. A container holds 0.320 m^3 of oxygen at an absolute pressure
of 6.00 atm. A valve is opened, allowing the gas to drive a piston,
increasing the volume of the gas until the pressure drops to 1.50
atm. If the temperature remains constant, what new volume does the
gas occupy?
2. Oxygen O2 molecules move with an rms speed of 452 m/s in a
gas. What is the temperature of the gas? Assume the gas is uniform
temperature throughout.

a) Consider molecules that are confined to move in a plane (a
two-dimensional gas). Calculate the distribution of speeds and
determine the mean speed of the molecules at a temperature T.
b) Evaluate numerically the fraction of O2
molecules with speeds in the range 100 m/s to 200 m/s in a gas at
300 K and 1000 K.

5. One mole of oxygen gas is at a pressure of 6.90 atm and a
temperature of 25.0°C.
(a) If the gas is heated at constant volume until the pressure
triples, what is the final temperature?
°C
(b) If the gas is heated so that both the pressure and volume are
doubled, what is the final temperature?
°C
6. (a) An ideal gas occupies a volume of 1.6 cm3 at
20°C and atmospheric pressure. Determine the number of molecules of...

Imagine you are sitting in a room full of oxygen molecules at
300 K. If the room has a volume of 1.0 x 104 m3, what is the number
of oxygen molecules in the room if the pressure is at 1 atm
(101,325 Pa)? Avogadro’s number is 6.02 x 1023 mol-1 and R = 8.31
J/mol-K.
a.
1.2 x 1028 molecules
b.
2.4 x 1028 molecules
c.
1.2 x 1029 molecules
d.
2.4 x 1029 molecules

A sealed container holds 0.020 moles of ideal nitrogen (N2) gas,
at a pressure of 1.5 atm and a temperature of 290 K. The atomic
mass of nitrogen is 14.0 g/mol. How many molecules of nitrogen are
in the container? (R = 8.31 J/mol • K, 1 atm = 101 kPa)

A mixture of methane gas, CH4(g), and pentane gas, C5H12(g), has
a pressure of 0.5015 atm when placed in a sealed container. The
complete combustion of the mixture to carbon dioxide gas, CO2(g),
and water vapor, H2O(g), was achieved by adding exactly enough
oxygen gas, O2(g), to the container. The pressure of the product
mixture in the sealed container is 2.421 atm. Calculate the mole
fraction of methane in the initial mixture assuming the temperature
and volume remain constant. Xch4=

A container holds 1.50 g of oxygen at a pressure of 6.00 atm
a. How much heat is required to increase the temperature by 101
∘C at constant pressure?
b. How much will the temperature increase if this amount of heat
energy is transferred to the gas at constant volume? (in C)

What volume of air contains 10.0 g of oxygen gas at 273 K and
1.00 atm?

A container holds 96.0 g of oxygen gas at a pressure of 8.00
atm. How much heat ? is required to increase the temperature by
80.0 ∘C at constant volume?

A gas in a container has an initial pressure of
0.637 atm. A chemical change occurs that consumes
a quarter of the molecules originally present and
forms three new molecules for every
four consumed. Determine the new pressure in the
container if the volume of the container and the temperature are
unchanged.
_____atm

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