Discussion Overview
The discussion revolves around the appropriate use of the ideal gas law and the van der Waals equation, specifically regarding the gas constant (R) and its units. Participants explore the implications of using different values of R in calculations, particularly in relation to pressure measurements in kPa and atm.
Discussion Character
- Debate/contested
- Technical explanation
- Mathematical reasoning
Main Points Raised
- Some participants note that R can be either 8.3145 J/(K·mol) or 0.082058 L·atm/(K·mol) and express confusion over the appropriate context for each value.
- One participant suggests that the gas constant for calculating pressure should be 0.082058 L·atm/(K·mol), arguing that the other value is more suited for thermodynamic calculations.
- Another participant mentions that both gas constants can be used, preferring kPa, and states that conversion between units is possible using the relationship 1 atm = 101.3 kPa.
- Some participants disagree on the applicability of the gas constants, with one asserting that there is a significant difference between the two constants based on their intended use in thermodynamics versus pressure calculations.
- Another participant counters that as long as units are consistent, the choice of gas constant should not affect the outcome of calculations.
- Several participants provide various values for the gas constant, indicating a range of accepted values and units.
Areas of Agreement / Disagreement
Participants express differing views on the appropriate use of the gas constants, with no consensus reached on whether one is definitively better for pressure calculations than the other. The discussion remains unresolved regarding the implications of using different constants in various contexts.
Contextual Notes
Participants highlight the importance of unit consistency when applying the ideal gas law and van der Waals equation, but there is no agreement on the necessity of using a specific gas constant for pressure calculations.
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