Question

Gases are often stored and shipped in high pressure containers. Consider a gas tank whose volume is 63.0 gallons and contains N2 gas at a pressure of 17,400 kPa at 21 degrees celsius. What is the mass of N2 contained in the tank? At what temperature would the pressure in the tank equal 145.0 atm?

Answer #1

Given that,

Volume of the gas V = 63.0 gallons = 63.0 * 3.785 L = 238.4 L

Pressure of the gas P = 17400 kPa = 17400 * 0.00987 atm = 171.74 atm

Temperature, T = 21 degree C = 21 + 273.15 = 294.15 K

number of moles, n = ?

Using Ideal gas equation,

P V = n R T

171.74 * 238.4 = n * 0.0821 * 294.15

n = 1695.4 mol

Mass / molar mass = 1695.4 mol

Mass of N2 = 1695.4 * 28 .00 = 47471.2 g.

*****

We know that,

P1 / T1 = P2 / T2

171.74 / 294.15 = 145.0 / T2

T2 = 248.35 K

t2 = 248.35 - 273.15 = - 24.80 degree C.

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