Question

A small gas cylinder containing CH4 (methane) gas is found to have a mass of 246.776g, and is used to bubble methane into a container that has been submerged in 22.0 C water. The volume of the gas that is inside the container at the end is 0.228L, and the gas cylinder weighs 246.622g. The barometric pressure of the room is 1.05atm.

1. Calculate the mass of CH4 that was released into the container.

2. Calculate the temperature of the water (and thus CH4 gas) in Kelvins.

3. Find the vapor pressure of water at this temperature.

4. Determine the partial pressure being exerted by the CH4 in the container in atm.

5. Use the ideal gas law and your calculated data above to calculate the number of moes of CH4 that were in the container.

6. Use the data from parts 1. and 5. to calculate the experimental molar mass of CH4

Answer #1

(1)

Mass of gas released into the container = Change in mass of
container = 246.776-246.622 = **0.154 g**

(2)

Temp of water and gas = 22^{0}C = 273+22 = **295
K**

(3)

Using the chart we see that vapor pressure of water at this temp
= 19.8 torr = **0.026 atm**

(4)

Pressure exerted by water + Pressure exerted by methane = 1.05 atm

So,

Pressure exerted by methane = 1.05-0.026 = **1.024
atm**

(5)

Using ideal gas equation:

PV = nRT

Putting values:

1.024*0.228 = n*0.0821*295

Solving we get:

n = **0.00964 moles**

(6)

Experimental molar mass = Mass/moles = 0.154/0.00964 =
**15.975 g**

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=

1. A sample of methane gas (CH4) at 24.4 oC is either heated or
cooled. The pressure increases from 1.21 atm to 3.80 atm, and the
volume of the sample changes from 1.02 L to 4.61 L. To what
temperature, in oC, was the methane heated or cooled?
2. An effusion container is filled with 5 L of an unknown gas.
It takes 321 s for the gas to effuse into a vacuum. From the same
container under the same...

Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and
an unknown amount of propane, C3H8) were added to the same 10.0-L
container. At 23.0 ∘C, the total pressure in the container is 4.40
atm . Calculate the partial pressure of each gas in the container.
Express the pressure values numerically in atmospheres, separated
by commas.
Enter the partial pressure of methane first, then ethane, then
propane.

Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and
an unknown amount of propane, C3H8) were added to the same 10.0-L
container. At 23.0 ∘C, the total pressure in the container is 4.40
atm . Calculate the partial pressure of each gas in the container.
Express the pressure values numerically in atmospheres, separated
by commas. Enter the partial pressure of methane first, then
ethane, then propane. A gaseous mixture of O2 and N2 contains 37.8
%...

Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and
an unknown amount of propane, C3H8) were added to the same 10.0-L
container. At 23.0 ∘C, the total pressure in the container is 5.30
atm . Calculate the partial pressure of each gas in the
container.

A 20.0 liter cylinder containing a mixture of oxygen and
nitrogen gas is sitting at room temperature (25.0 oC).
Given that the mole fraction of nitrogen is 0.24, and the partial
pressure of oxygen is 1.60 atm, what is the total pressure of the
gas mixture in this container?

A sample of 64.0 g of methane, CH4 (molecular mass
16.0 g/mol, assume ideal gas behaviour)) at 300 K and with an
initial pressure V1 = 1.00 m3 is
compressed isothermally and reversibly to a final volume
of 2.00L. Calculate DU, DH, w, and q

A flask with a sample of gas at room temperature and pressure
weighs 97.4842 g. The same flask with air (density = 1.17 g/L)
weighs 96.8848 g. The same flask filled with water (d = 0.998 g/mL)
weighs 345.86 g. The pressure in the room is 0.989 atm and the
temperature is 22.2 °C.
1. Calculate the volume of the flask.
2. Calculate the mass of the air that the flask can hold.
3. Calculate the mass of the empty...

Nitrogen gas reacts with hydrogen gas to form ammonia gas . You
have nitrogen and hydrogen gases in a -L container fitted with a
movable piston (the piston allows the container volume to change so
as to keep the pressure constant inside the container). Initially
the partial pressure of each reactant gas is atm. Assume the
temperature is constant and that the reaction goes to completion.
Calculate the partial pressure of ammonia in the container after
the reaction has reached...

A cylinder of compressed gas rolls off a boat and falls to the
bottom of a lake. Eventually it rusts and the gas bubbles to the
surface. A chemist collects a sample of the gas with the idea of
trying to identify the gas. The wet gas collected occupies a volume
of 287 mL at a pressure of 722 torr and temperature of 28.0oC. The
vapor pressure of water at 28.0oC is 0.0372 atm.
1. Calculate the volume (L) that...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 1 minute ago

asked 1 minute ago

asked 1 minute ago

asked 1 minute ago

asked 2 minutes ago

asked 3 minutes ago

asked 7 minutes ago

asked 7 minutes ago

asked 11 minutes ago

asked 11 minutes ago

asked 11 minutes ago

asked 12 minutes ago