Question

At temperature of 273 K and pressure of 1.00 × 10−2 atm, the density of a monatomic gas is 1.24 × 10−5g/cm3.

Also, we know 1 atm = 1.01 × 105 Pa, R = 8.31 J/mol.K and ? = 1.38 × 10−23 J/K.

(a) Find ???? for the gas particles.

(b) Find the molar mass of the gas.

Answer #1

The volume of an ideal gas is adiabatically reduced from 200 L
to 74.3 L. The initial pressure and temperature are 1.00 atm and
300 K. The final pressure is 4.00 atm.
? = 8.314 J/mol.K , ????????? = 1.4, ??????????? = 1.67 and 1
atm = 1.013 × 10^5 Pa. mol.K
(a) Is the gas monatomic or diatomic?
(b) What is the final temperature?
(c) How many moles are in the gas?

1) At standard temperature and pressure (0 ∘C and 1.00 atm ),
1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume
would the same amount of gas occupy at the same pressure and 45 ∘C
?
Express your answer with the appropriate units.
2) One mole of an ideal gas is sealed in a 22.4-L container at a
pressure of 1 atm and a temperature of 273 K. The temperature is
then increased to 304...

A rigid cubic container of side 0.25 m is filled with 10 moles
of the ideal gas Xenon and is then sealed so that no gas can get
out or in. The initial pressure of the gas is recorded as 2.8 x
105 Pa. You may use the following values for this
question:
Gas constant R: 8.31 J/(mol K)
Boltzmann constant kB : 1.38 x 10-23
J/K
Avogadro's number NA: 6.02 x 1023 /mol
A) Determine the total amount of...

One mole of an ideal gas does 3000 J of work on its surroundings
as it expands isothermally to a final pressure of 1.00 atm and
volume of 25.0 L. Determine:
a) the initial volume ?
b) the temperature of the gas?
(Note: 1 atm = 1.01 x 105Pa, universal gas constant R
= 8.31 J/mol K, 1 L = 10-3m3)

4. Three moles of a monatomic ideal gas are initially at a
pressure of 1.00 atm and a temperature of 20.0OC. The gas is
compressed adiabatically to a final pressure of 5.00 atm. Find: (a)
the initial volume of the gas; (b) the final volume of the gas; (c)
the final temperature of the gas; (d) the work done by the gas
during the compression.
Answers: (a) 72.1 L; (b) 27.5 L; (c) 285 OC; (d) -97.8
atm-L
Please show...

You are given an ideal monatomic gas of N = 1.00 × 1023 atoms at
temperature T = 300K, and volumeV = 20 L. Find:
(a) The pressure in the gas in Pa.
(b) The work done in Joules when the gas is compressed slowly
and isothermally to half its volume.
(c) The change in internal energy of the gas in Joules during
process (b).
(d) The heat (in J) absorbed or given up by the gas during
process (b)....

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...

An ideal monatomic gas expands isothermally from 0.600 m3 to
1.25 m3 at a constant temperature of 730 K. If the initial pressure
is 1.02 ? 105 Pa find the following.
(a) the work done on the gas
J
(b) the thermal energy transfer Q
J
(c) the change in the internal energy
J

A vessel with a movable piston contains 1.90 mol of an ideal gas
with initial pressure
Pi = 2.03 ✕ 105 Pa,
initial volume
Vi = 1.00 ✕ 10−2
m3,
and initial temperature
Ti = 128 K.
(a) What is the work done on the gas during a constant-pressure
compression, after which the final volume of the gas is 2.50
L?
J
(b) What is the work done on the gas during an isothermal
compression, after which the final pressure...

n = 3.50 mol of Hydrogen gas is initially at T = 309.0 K
temperature and pi = 2.34×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 8.91×105 Pa.
1. What is the volume of the gas at the end of the compression
process? 1.01×10-2
m^3
2. How much work did the external force perform?
3. How much heat did the gas emit?
4. How much entropy did the gas emit?
5....

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