14. PV nRT in all its possible uses. Here are a few examples of the many possibl

Question

14. PV nRT in all its possible uses. Here are a few examples of the many possible. A. A sample of Argon gas occupies a 1.5 L cylinder at a temperature of 22 °C. The cylinder has a pressure of 125 atm. How many moles of argon occupy the cylinder? B. A 5.0 L cylinder is filled with 34.0 moles of nitrogen gas at 293 °C, calculate the pressure in the cylinder in atm C. High pressure chemistry is conducted in a vessel commonly called a "bomb". A 1.25 L bomb is pressurized to 1,500 psi and sealed room temperature (23 °C). If the temperature is raised to 450 °C, what is the final pressure in psi and atm. D. A gas filled balloon having a volume of 2.50 L at 1.2 atm and 25 °C is allowed to rise to the stratosphere (about 30 km above the surface of the Earth), where the temperature and pressure is 23 °C and 3.00 x 10' atm, respectively. Calculate the final volume of the balloon. E. IfI have a sealed steal cylinder containing an inert gas and I increase the pressure what effect will this have?

Explanation / Answer

(A)

n = P V / R T

n = 125 * 1.5 / (0.0821 * 295.15)

n = 7.74 mol

(B)
T = 293 + 273.15 = 566.15 K

P = n R T/ V

P = 34.0 * 0.0821 * 566.15 / 5.0

P = 316. atm

(C)

P1 = 1500 psi

T1 = 23 + 273.15 = 296.15 K

P2 = ?

T2 = 450 + 273.15 = 723.15 K

P1 / T1 = P2 / T2

1500 / 296.15 = P2 / 723.15

P2 = 3663. psi

P2 = 3663 * 0.0680 atm = 249. atm

D.

P1 = 12. atm

V1 = 2.50 L

T1 = 25 + 273.15 = 298.15 K

P2 = 0.00300 atm

T2 = - 23 + 273.15 = 250.15 K

V2 = ?

Formula,

P1 * V1 / T1 = P2 * V2 / T2

1.2 * 2.50 / 298.15 = 0.00300 * V2 / 250.15

V2 = final volume = 839. L

E.

It will increase the tmeperature.

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