A chemical engineering question, can someone help? An oxygen cylinder used as a

Question

A chemical engineering question, can someone help? An oxygen cylinder used as a standby source of oxygen contains 1.000 ft^3 of O_2 at 70 degree F and 200 psig. The barometer reads 29.92 in. Hg. Assume ideal gas behavior. a) What is the number of moles of O2 contained in the cylinder. b) What will be the volume of this O_2 in a dry-gas holder at 90 degree F and 4.00 in. H_2O above atmospheric? c) Where do you think the ideal gas behavior is more justified, at the initial condition or the final condition? Explain your answer.

Explanation / Answer

Hi

a) P= 200 psig = 13.61 atm

V= 1 ft^3 = 28.32 L

T= 70 F= 294.26 K

n= PV/RT = (13.61*28.32)/(0.082*294.26) = 15.974 gmoles

b) P= 4*0.0254*9.8*1000 = 995.68 Pa

T= 90 F= 305.372 K

V= nRT/P = (15.974*8.314*305.372)/995.68 m^3

V= 40.732 m^3 = 40732 L

c) The ideal gas behaviour is more justified in final condition. Since, the gases tend to follow ideal behaviour at low pressure and high temperature and both the conditions are present in final condition.

Thank you

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.