Question

what pressure will be required for neon at 30.0C to have the same density as nitrogen at 20.0C and at 1.00 atm? state your final answers in atm unit using 3 SF's

Answer #1

Density of Nitrogen at 20.0 C = m/V =
P_{N2}M_{N2}/RT_{N2}

[ P_{N2}=pressure of nitrogen, M_{N2}= molar
mass of nitrogen, R=Universal const, T_{N2}= temperature of
nitrogen]

= (1 atm x 28 g mol^{-1})/ ( 0.082 L atm K^{-1}
mol^{-1} x 293.15 K)

= 1.16 g L^{-1}

Similarly we can write, density of Neon =
P_{Ne}M_{Ne}/RT_{Ne} here terms have usual
meanings (molar mas =20 g mol^{-1})

We know density is 1.16 g/L , 1.16 g/L
= (P_{Ne} x 20 g mol^{-1}) / (0.082 L atm
K^{-1} mol^{-1} x 303.15 K)

**P _{Ne} = 1.44 atm**

This should be the pressure at which density will be same.

A) What is the density of neon gas at 64.5 ∘C and 3.70 atm?
B) At a different temperature and pressure neon gas was
determined to have a density of 1.65 g/L. What is the density of
sulfur hexafluoride gas at this new temperature and pressure?

A tank contains helium gas at 490. mmHg, nitrogen gas at 0.750
atm, and neon at 520. Torr. What is the total pressure in atm?
A) 2.08 atm B) 0.579
atm C) 1.01 × 103
atm D) 1.33
atm E) 1.60 ×
103 atm How is this done please?

A steel cylinder with a volume of 15.0 L is filled with 69.4 g
of nitrogen gas at 25∘C.
Part A
What is the pressure, in atmospheres, of the N2 gas in the
cylinder?
Express your answer to three significant figures with the
appropriate units.
-------------------------------------------------------------------------------------------------------------------------------
Part B
How many liters of H2 gas can be produced at 0 ∘C and 1.00 atm
(STP) from 44.5 g of Zn?
Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g)
Express your answer with the appropriate units.
----------------------------------------------------------------------------------------------------------------------------------------------------------------------
A gas...

Nitrogen, N2, is soluble in blood and can cause intoxication at
sufficient concentration. For this reason, the U.S. Navy advises
divers using compressed air not to go below 125 feet. The total
pressure at this depth is 4.79 atm. If the solubility of nitrogen
at 1.00 atm is 1.75E-3 g/100 mL of water, and the mole percent of
nitrogen in air is 78.1, what is the solubility of nitrogen in
water from air at 4.79 atm?

You have equal masses of neon gas and argon gas in a 100 L
vessel at 3.731 atm and 25*C.
a. What is the total mass of gas in the vessel?
Consider that the gas is heated to 118.5*C in two possible
ways.
a. The gas is heated to 118.5*C in a rigid container such that
the volume is constant. Determine the partial pressure of the neon
gas in such a container.
b. The gas is heated to 118.5*C in...

A) The solubility of neon gas in water at 25°C is 1.05x10-3 M when
the pressure of the Ne above the solution is 1.0 atm. the
solubility of Ne (g) is?
B) the vapor pressure of pure ethanol at 60°C is 0.459 atm.
Raoult's law predicts that a solution prepared by dissolving 10.0
mmol naphthalene in 90.0 mmol ethanol will have a vapor pressure
of?

Estimate the mass and volume of nitrogen gas required to
pressurize an N O − MMH feed 24 system for a 4500 N thrust chamber
of 25 sec duration (?? = 0.92, the ideal Is = 285 sec at 1000 psi
or 6894 N/m2 and expansion to 1 atm).
The chamber pressure is 20 atm (absolute) and the mixture ratio
is 1.65.
The propellant tank pressure is 30 atm, and the initial gas tank
pressure is 150 atm.
Allow for...

A
storage tank contains 15 kg of nitrogen at an absolute pressure of
4.35 atm. What will the pressure be if the nitrogen is replaced by
an equal mass of CO2 in atm? (Molecular mass of nitrogen and carbon
is 28.01u and 44.01u)
How
many molecules of carbon dioxide are in the tank?
How
much additional carbon dioxide should be added to the tank to
regain the original pressure in kg?

That is, select "1" next to the sample in which the neon atoms
have the lowest average kinetic energy. Select "2" next to the
sample in which the neon atoms have the next lowest average kinetic
energy, and so on.
please show me steps..
sample
Amount
Pressure
Temperature
1
1.5 mole
1.0 atm
-20 C
2
2.1 mole
1.3 atm
19 C
3
1.1 mole
1.7 atm
6 C
4
2.0 mole
2.4 atm
2 C
5
2.6 mole
2.0...

Initially 5 mole of
nitrogen are at a temperature of 25. Degrees C and a pressure of
10.0 bar. Cv,m=20.8
J K-1
mol-1
and is
independent of temperature. Suppose the pressure is
suddenly dropped to 1.00
bar. Calculate the final temperature, U, q, w, and
H. State any
assumptions that you make

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