Question

A tank with a volume of 8.6 ft3 contains 5.36 lbmol of carbon monoxide (CO) gas at a pressure of 3500 lbf/in.2 Determine the temperature, in °R. Determine the percent error in temperature of assuming ideal gas behavior at this state for CO.

Please provide the complete answer.

Answer #2

First, let us convert all the values into SI units.

Pressure, P = 3500 lbf/in^{2} = 241.3 bar = 241.3 x
10^{5} N/m^{2}

Volume, V = 8.6 ft^{3} = 0.244 m^{3}

5.36 lbmol = 2431.26 mol

Universal Gas Constant, R = 8.314 J/K/mol

We know that,

PV = nRT,

putting values and solving for T, we have,

T = [(241.3 x 10^{5})x0.244]/[8.314 x 2431.26] =
291.26K

Now converting unit into degree Rankine, we have T = 524.28°R

Ideal gas temp = 273K = 491.4°R

Calculating % error = (524.28 - 491.4)/491.4 x 100 = 6.72% error. Ans.

answered by: anonymous

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