Question

If 35.5 moles of an ideal gas occupies 53.5 liters at 411 K, what is the pressure of the gas?

If 54.5 mol of an ideal gas is at 1.29 atm and 337 K, what is the volume of the gas?

Answer #1

For an ideal gas, calculate the following quantities.
(a) The pressure of the gas if 0.135 mol occupies 207 mL at
25°C.
______atm
(b) The temperature (in kelvins) at which 0.0250 mol occupies
1.00 L at 0.563 atm. K (c) The number of moles in 4.50 L at -7°C
and 715 torr. Remember 1atm = 760 torr.
_____mol
(d) The volume occupied by 4.72 10-3 mol at 40.°C and a pressure
of 1.57 kPa. Remember 1 atm = 101.325 kPa...

1/ A sample of xenon gas that occupies a volume
of 42.7 L at a temperature of 0 °C and a pressure
of 1 atm contains (......) moles of gas.
2/ A sample of nitrogen gas collected at STP
occupies a volume of 13.4 L. How many moles of gas
does the sample contain? (.......) mol
3/ What volume is occupied by a 0.920 mol
sample of carbon dioxide gas at a temperature of 0
°C and a pressure of...

For an ideal gas, calculate the following quantities.
(a) The pressure of the gas if 0.135 mol occupies 207 mL at
35°C.
_____atm
(b) The temperature (in kelvins) at which 0.0260 mol occupies
3.00 L at 0.563 atm.
__________K
(c) The number of moles in 5.00 L at -2°C and 735 torr. Remember
1atm = 760 torr.
_________mol
(d) The volume occupied by 6.72 10-3 mol at 20.°C and a pressure
of 1.77 kPa. Remember 1 atm = 101.325 kPa...

A sample of ideal gas at room temperature occupies a volume of
36.0 L at a pressure of 692 torr . If the pressure changes to 3460
torr , with no change in the temperature or moles of gas, what is
the new volume, V2?

2.50 Liters of CO2 gas (ideal) at 25^{\circ }C and 1.o atm of
pressure is allowed to expand in volume until the final pressure
and temperature are 0.50 atm and 15^{\circ }C , respectively:
a) Calculate the final volume of the gas.
b) Calculate the # of moles, n, of the gas.
c) Calculate the # of grams of the gas.

3 moles of a monoatomic ideal gas with Cv=(32)RT occupies a
volume of 3.2L at a pressure of 1.9atm at point A. The gas is
carried through a cycle consisting of three processes:
1. The gas is heated at constant pressure until its volume is 4.4L
at point B.
2. The gas is cooled at constant volume until the pressure
decreases to 1.2atm (C).
3. The gas undergoes an isothermal compression back to point
A.
Find W for the isochoric...

An ideal gas at 10.0 °C and a pressure of 2.75 x 105
Pa occupies a volume of 3.49 m3. (a)
How many moles of gas are present? (b) If the
volume is raised to 5.63 m3 and the temperature raised
to 29.2 °C, what will be the pressure of the gas?

If an ideal gas has a pressure of 8.15 atm, a temperature of
387 K, and a volume of 99.07 L, how many moles of gas are in the
sample?

A sample consisting of 2.5 moles of ideal gas (Cp,m
=20.8 J/K) is initially at 3.25 atm and 300 K. It undergoes
reversible adiabatic expansion until its pressure reaches 2.5 atm.
Calculate the final volume, the final temperature, and the work
done.

if
20.5 mol of an ideal gas is at 6.83 atm and 319 K, what is the
volume of the gas?

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