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Compressibility factor for CO2 at 400 K and 71.0 bars Video Lecture - Class 12
FAQs on Compressibility factor for CO2 at 400 K and 71.0 bars Video Lecture - Class 12
| 1. What is the formula to calculate the compressibility factor for CO2 at a given temperature and pressure? |  |
Ans. The compressibility factor (Z) for a gas can be calculated using the formula Z = PV/RT, where P is the pressure, V is the molar volume, R is the gas constant, and T is the temperature.
| 2. How does the compressibility factor affect the behavior of CO2 at 400 K and 71.0 bars? | |
Ans. The compressibility factor provides information about the deviation of a gas from ideal behavior. If the compressibility factor is close to 1, the gas behaves ideally. If it is greater than 1, the gas exhibits attractive forces between molecules and deviates from ideal behavior. If it is less than 1, the gas exhibits repulsive forces between molecules and also deviates from ideal behavior.
| 3. What are the units of the compressibility factor? | |
Ans. The compressibility factor is a dimensionless quantity and does not have any units. It is simply a ratio of the actual volume of a gas to the ideal volume predicted by the ideal gas law.
| 4. How can the compressibility factor be used to determine the phase of CO2 at 400 K and 71.0 bars? | |
Ans. The compressibility factor can provide information about the phase of a gas at a given temperature and pressure. If the compressibility factor is close to 1, it indicates that the gas is in the gaseous phase. If it is significantly higher or lower than 1, it suggests that the gas may be in a condensed phase such as a liquid or solid.
| 5. Can the compressibility factor be used to predict the behavior of other gases at the same conditions? | |
Ans. Yes, the compressibility factor can be used to predict the behavior of other gases at the same temperature and pressure conditions. By calculating the compressibility factor for different gases, one can compare their deviations from ideal behavior and determine whether they exhibit attractive or repulsive forces between molecules. This information is useful in various fields such as chemical engineering, thermodynamics, and gas phase reactions.
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