Question

On a hot summer day, the density of air at atmospheric pressure at 34.5°C is 1.1242 kg/m3.

(a) What is the number of moles contained in 1.00 m3 of an ideal gas at this temperature and pressure? mol

(b) Avogadro's number of air molecules has a mass of 2.82 ✕ 10−2 kg. What is the mass of 1.00 m3 of air? (Assume air is an ideal gas.) kg

(c) Does the value calculated in part (b) agree with the stated density of air at this temperature? (Consider that it does if the values are within 10% of each other.) Yes or no?

Answer #1

On a warm summer day, a large mass of air (atmospheric pressure
1.01×105Pa) is heated by the ground to a temperature of 26.0 ∘C and
then begins to rise through the cooler surrounding air.
1.Calculate the temperature of the air mass when it has risen to
a level at which atmospheric pressure is only 8.60×104
Pa . Assume that air is an ideal gas, with γ=1.40. (This
rate of cooling for dry, rising air, corresponding to roughly 1 ∘C
per...

The density of uncompressed air is 1.293 kg/m3, and
one mole of air (containing Avogadro's number of molecules) has a
mass of 28.94 g.
a) Use the density and the volume of the uncompressed air 45 cc to
determine the mass of the air in the syringe,
mair, in grams. (You will have to do some unit
conversions.)
mair = ______ g
b)Use the mass of one mole of air and Avogadro's number to
determine N, the number of molecules in...

If the molecular weight of air is 28.9, what is the density of
air at atmospheric pressure and a temperature of 368.7 K? 1 atm =
1.013×105 N/m2, the mass of a proton is 1.67262 × 10?27 kg ,
Avogadro’s number is 6.02214 × 1023 mol?1 and k = 1.38065 × 10?23 N
· m/K . Answer in units of kg/m3.

Air (a diatomic ideal gas) at 26.5°C and atmospheric pressure is
drawn into a bicycle pump (see figure below) that has a cylinder
with an inner diameter of 2.50 cm and length 47.0 cm. The
downstroke adiabatically compresses the air, which reaches a gauge
pressure of 8.00 105 Pa before entering the tire. We wish to
investigate the temperature increase of the pump.
The pump is made of steel that is 1.80 mm thick. Assume 4.00 cm
of the cylinder's...

1.How many air molecules are in a 14.5×12.0×10.0 ft room? Assume
atmospheric pressure of 1.00 atm, a room temperature of 20.0 ∘C,
and ideal behavior. Volume conversion:There are
28.2 liters in one cubic foot.
2. At an underwater depth of 255 ft , the pressure is 8.33
atm
What should the mole percent of oxygen be in the diving gas for
the partial pressure of oxygen in the mixture to be 0.21 atm, the
same as in air at 1...

How many air molecules are in a 15.0×12.0×10.0 ft room? Assume
atmospheric pressure of 1.00 atm, a room temperature of 20.0 ∘C,
and ideal behavior. Volume conversion:There are 28.2 liters in one
cubic foot.

Calculate the temperature and the density of atmospheric air
at 3600 m altitude, when the field of atmospheric pressures is
given by the expression:
p = p0 (1 - cz) ^(5.25)
where z is the altitude,and p0 and c are constants
p0 = 0.1x10^6Pa
c = 0.021km^(-1).
Consider the air as an ideal gas of molar mass M =
0.029kg/mol

Air with a mass of 2 kg is heated at a constant pressure of
200 kPa to a temperature
of 500°C. Calculate the entropy change if the initial volume
is 0.8 m3. Take ???? =
1.00 kJ/kg ? K and model air as an ideal gas. (Hint: Use the
appropriate TdS [Gibbs] relation to calculate entropy
change.)

The air in a hot-air balloon at 786 torr is heated from 19.0°C
to 33.0°C. Assuming that the moles of air and the pressure remain
constant, what is the density of the air at each temperature? (The
average molar mass of air is 29.0 g/mol.) Density at 19.0°C =
Density at 33.0°C=

1) A hot air balloon consists of a very large bag filled with
heated air at 120.0 °C produced from a propane burner. It has a
basket hanging under it in which several people can ride. The
average hot air balloon has a volume of 2.80 × 103 m3 when fully
inflated.
a) Determine the work (in kJ) needed to inflate the balloon under
an external air pressure of 1.00 atm.
b) The specific heat of the air found in...

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