Why doesn't (P1xV1)/T1 = (P2xV2)/T2 work here?

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In summary, the pressure-temperature-volume relationship, also known as the ideal gas law, may not be applicable in certain situations where real gases or non-ideal conditions are present. Factors such as intermolecular forces, non-ideal gas behavior, and changes in temperature, pressure, or volume can affect the accuracy of this relationship. It is only applicable for ideal gases under ideal conditions and an alternative equation, such as the van der Waals equation, may be used in situations where it does not work. To determine if the relationship is applicable, the gas's behavior can be compared to that of an ideal gas using parameters like temperature, pressure, and volume.
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eurekameh
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10 kg of R-134a fill a 1.348 m^3 rigid container at an initial temperature of -40 degrees Celsius. The container is then heated until the pressure is 200 kPa. Determine the final temperature and the initial pressure.

I found the final temperature to be 66.3 degrees Celsius and the initial pressure to be 51.25 kPa using thermodynamic property tables. However, when I plugged all of the values into the equation (P1 x V1)/T1 = (P2xV2)/T2, it does not work. Can anyone explain why?
 
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  • #2
Would you expect it to behave as an ideal gas over that temperature range?
 
  • #3
ahh. i see. thanks =)
 

Related to Why doesn't (P1xV1)/T1 = (P2xV2)/T2 work here?

1. Why is the pressure-temperature-volume relationship not applicable in this situation?

The pressure-temperature-volume relationship, also known as the ideal gas law, is based on the assumption that the gas behaves ideally without any intermolecular forces. However, in certain situations, such as when dealing with real gases or non-ideal conditions, this assumption may not hold true and therefore the relationship may not be applicable.

2. What factors can affect the accuracy of the pressure-temperature-volume relationship?

The accuracy of the pressure-temperature-volume relationship can be affected by several factors, such as the presence of intermolecular forces, non-ideal gas behavior, and changes in the gas's temperature, pressure, or volume. Other factors like the type of gas, the container's material, and any external factors can also impact the accuracy of the relationship.

3. Can the pressure-temperature-volume relationship be used for all types of gases?

No, the pressure-temperature-volume relationship is only applicable for ideal gases under ideal conditions. Real gases, which have intermolecular forces and do not behave ideally, may not follow this relationship. Additionally, different types of gases have different properties and may not behave in the same way under the same conditions.

4. Is there an alternative equation that can be used in situations where the pressure-temperature-volume relationship does not work?

Yes, the van der Waals equation is an alternative equation that can be used for real gases or non-ideal conditions. It takes into account the intermolecular forces and the finite size of gas molecules, making it a more accurate representation of gas behavior in these situations.

5. How can we determine if the pressure-temperature-volume relationship is applicable in a given situation?

The pressure-temperature-volume relationship is applicable when the gas behaves ideally, which means that the gas molecules have negligible volume and do not interact with each other. In order to determine this, the gas's behavior can be compared to that of an ideal gas using various parameters such as temperature, pressure, and volume. If the gas's behavior is similar to an ideal gas, then the relationship can be used. Otherwise, an alternative equation, such as the van der Waals equation, may be more appropriate.

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