Solution Found!
Working with the Ideal Gas ModelA tank contains 0.5 m3 of
Chapter 3, Problem 100P(choose chapter or problem)
A tank contains \(0.5 \mathrm{~m}^3\) of nitrogen \(\left(\mathrm{N}_2\right)\) at \(-71^{\circ} \mathrm{C}\) and \(1356 \mathrm{kPa}\). Determine the mass of nitrogen, in kg, using
(a) the ideal gas model.
(b) data from the compressibility chart.
Comment on the applicability of the ideal gas model for nitrogen at this state.
Questions & Answers
QUESTION:
A tank contains \(0.5 \mathrm{~m}^3\) of nitrogen \(\left(\mathrm{N}_2\right)\) at \(-71^{\circ} \mathrm{C}\) and \(1356 \mathrm{kPa}\). Determine the mass of nitrogen, in kg, using
(a) the ideal gas model.
(b) data from the compressibility chart.
Comment on the applicability of the ideal gas model for nitrogen at this state.
ANSWER:Step 1 of 3
We have to determine the mass of nitrogen in a tank which contains 0.5 m3 of nitrogen (N2) at −71°C and 1356 kPa using the ideal gas model and also by the data from the compressibility chart.
The equation of state according to ideal gas model is given by
or
where, mass of nitrogen in kg
Volume of nitrogen = 0.5 m3
gas constant =8.314 kJ/kmol
K
pressure of nitrogen = 1356 kPa
Temperature of the nitrogen = -71 oC = 202.15 K
Thus,
1356
= 0.403 kg
Therefore, the mass of nitrogen from the ideal gas model is 0.403 kg.
b.)