Question

Given PV=0.08206nT answer the following:

A- Convert the equation to one relating P(psig),V(ft^3),n(ln-mole), and T(Fehrenheit).

B- A 30 mole% CO and 70 mole% N2 gas mixture is stored in a cylinder with a volume of 3.5ft^3 at a temperature of 85F. The reading on a bourdon gauge attached to the cylinder is 500 psi. Calculate the total amount of gas (lb-mole) and the mass of CO (lbm) in the tank

C- Approximately to what termperature (F) would the cylinder have to be heated to increase the gas pressure to 3000 psig, the rated safety limit of the cylinder?( the estimate would only be approximate because the ideal gas equation of state would not be accurate at pressure this high.)

Answer 1

A.

In the equation PV = 0.08206 L-atm/mole* Kelvin * nT, the units for R show that P is in atm, V is in litres and T is in kelvin

1 atm = 14.6959 Psig

1 litre = 1 m³ and 1 m³ = 35.3147 ft³

0 Kelvin = 273.15 ⁰C and 0 ⁰C = 32 F

==> So 0 Kelvin = -459.67 F

Substituting these values into PV = nRT equation, we get

(14.6959 Psig) (35.3147 ft^{3) =} n * (10.73159) * (-459.67)

10.73159 is the ideal gas constant, in ft³·psi / °R·lb-mol
n is the mass, in lb-mol

***For next set of questions, please submit them as separate questions as they are enough lengthy and calculative