Question Solved1 Answer 3.67. As will be discussed in detail in Chapter 5, the ideal-gas equation of state relates absolute pressure, P(atm); gas volume, V(liters); number of moles of gas, n(mol); and absolute temperature, T(K): (a) Convert the equation to one relating P(psig), V(ft) n(lb-mole), and TCD. (b) A 30.0 mole% CO and 70.0 mole% N2 gas mixture is stored in a cylinder with 3.67. As will be discussed in detail in Chapter 5, the ideal-gas equation of state relates absolute pressure, P(atm); gas volume, V(liters); number of moles of gas, n(mol); and absolute temperature, T(K): (a) Convert the equation to one relating P(psig), V(ft) n(lb-mole), and TCD. (b) A 30.0 mole% CO and 70.0 mole% N2 gas mixture is stored in a cylinder with a volume of 3.5 ta a temperature of 85°F. 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. (e) Approximately to what temperature (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 pressures this high.)

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Transcribed Image Text: 3.67. As will be discussed in detail in Chapter 5, the ideal-gas equation of state relates absolute pressure, P(atm); gas volume, V(liters); number of moles of gas, n(mol); and absolute temperature, T(K): (a) Convert the equation to one relating P(psig), V(ft) n(lb-mole), and TCD. (b) A 30.0 mole% CO and 70.0 mole% N2 gas mixture is stored in a cylinder with a volume of 3.5 ta a temperature of 85°F. 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. (e) Approximately to what temperature (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 pressures this high.)
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Transcribed Image Text: 3.67. As will be discussed in detail in Chapter 5, the ideal-gas equation of state relates absolute pressure, P(atm); gas volume, V(liters); number of moles of gas, n(mol); and absolute temperature, T(K): (a) Convert the equation to one relating P(psig), V(ft) n(lb-mole), and TCD. (b) A 30.0 mole% CO and 70.0 mole% N2 gas mixture is stored in a cylinder with a volume of 3.5 ta a temperature of 85°F. 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. (e) Approximately to what temperature (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 pressures this high.)
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(a) Conversions: 1 atm=14.696 psig, 1 ft3=28.317 L, 1 lb mol=453.59 mol Convert the units of each term P( atm )=(P^(')(p sig)+14.696)/(14.696) V(L)=V^(')(ft^(3))**28.317 ft^(3)//L n(mol)=n^(')(lbmol)**453.59mol//lbmol T(K)=(T^(')(^(@)F)-32)/(1.8)+273.15 The ideal gas equation is PV=0.08206 nT =>(P^(')+14.696)/(14.696)**V^(')**28.317=0.08206**n^(')**453.59**((T^(')-32)/(1.8)+273.15) where P' is the Pressure in psig V' is the Volume in ft3 n' is the Number of moles in lb mol T' is the Temperature in 0F =>(P^(')+14.696)**V^(')=(14.696**0.08206**453.59)/(28.317**1.8)**n^(')**(T^(')-32+491.67) (P^(')+14.696)V^(')=10.7318n^(')(T^(')+459.67) (b) Given: Mole fraction of CO, xCO=30 mole%=0.30 lb mole CO/lb mole Mole fraction of N2, xN2=70 mole%=0.70 lb mole N2/lb mole Volume of the cylinder, V=3.5 ft3 Temperature, T=850F Bourdon ... See the full answer