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Questions and Answers
At extremely low pressures and high temperatures, what happens to the correction terms (b) and (a/V^2) of the Van der Waals equation?
At extremely low pressures and high temperatures, what happens to the correction terms (b) and (a/V^2) of the Van der Waals equation?
What is the reason why PV for H2 begins to increase sharply with an increase of pressure?
What is the reason why PV for H2 begins to increase sharply with an increase of pressure?
How can every gas be converted into a liquid state?
How can every gas be converted into a liquid state?
In which method is gas liquefaction achieved through the Joule-Thomson effect?
In which method is gas liquefaction achieved through the Joule-Thomson effect?
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What is the critical temperature (Tc) defined as?
What is the critical temperature (Tc) defined as?
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Study Notes
Van der Waals Equation
- The Van der Waals equation for 1 mole is: 𝒂𝒂 𝑷𝑷 + 𝟐𝟐 𝑽𝑽 − 𝒃𝒃 = 𝑹𝑹𝑹𝑹 𝑽𝑽
- The equation can be rearranged to: 𝑷𝑷𝑷𝑷 − 𝒃𝒃𝒃𝒃 + 𝒂𝒂⁄ 𝑽𝑽 𝒂𝒂𝒂𝒂 = 𝑹𝑹𝑹𝑹
Behavior of Real Gases at Low Pressure
- At low pressure, P is small, and V is large
- The terms Pb and ( ab/V2 ) are negligible values
- As P increases, V decreases, and (a/V) increases; therefore, PV will decrease
- This explains the dip part in the plot of PV vs P for gases such as CO2 and N2
Behavior of Real Gases at High Pressure
- At high pressure, P is high, and V is small
- The terms (a/V) and ( ab/V2 ) cancel each other out
- As P increases, Pb increases; therefore, PV will increase
- This explains the positive deviation part in the plot of PV vs P for gases such as CO2 and N2
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Description
Test your understanding of the behavior of real gases with this quiz on the Van der Waals equation. Explore how the equation describes the deviations of real gases from ideal behavior and solve problems related to pressure, volume, and gas constants.
