Why don\'t real gases behave ideally at very low temperatures? In Part A, what i

Question

Why don't real gases behave ideally at very low temperatures? In Part A, what is the pressure of the air inside the flask? Can we assume this pressure is constant throughout the experiment? Based on your Group Data in Part A, calculate the air density (in g/L) when: i) your flask was immersed in the boiling water bath; and ii) your flask was immersed in your group's cool water bath. (M_dry air = 29.0 g/mol) Explain how each of the following errors in Part B would affect the calculation of the molar mass of the unknown. a. Heating was stopped before all of the liquid in the flask had evaporated (Step 10). b. Water remained on flask and stopper assembly when the mass of the condensed liquid was the outside of the determined (Step 12) c. The volume of the Erlenmeyer flask was assumed to be 125-mL and not measured as directed (Step 14).

Explanation / Answer

1. Real gases differ from ideal gases due to two reasons:-

A. Unlike ideal gases volume occupied by real gas molecules cannot be neglected in comparison to total volumes of gases

B. Unlike ideal gases there are interactions between molecules of real gases

At very low temperature the interactions between gases are significant so real gas differ from the ideal behaviour

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