9. Consider the following gases: (a) H20 at 375 K and 750 torr (b) He at 37.5 K
ID: 569885 • Letter: 9
Question
9. Consider the following gases: (a) H20 at 375 K and 750 torr (b) He at 37.5 K and 7500 torr (c) CH4 at 37.5 C and 7.5 atnm (d) Ne at 375 °C and 0.75 atm (e) SFo at -37.5 C and 0.75 atm Which gas is most likely to behave as an ideal gas? Explain NOTE: Your answer for question 9 must include at least five sentences and will be graded for scientific accuracy and completeness. It also will be assessed for organization, clarity, spelling, grammar, and punctuation. The latter may contribute to bonus marks on your final course gradeExplanation / Answer
Ans. Converts all temperatures and pressure in terms of kelvin and atm, respectively.
#a. H2O at 375 K and 750 torr
Pressure, P = (750 / 760) atm = 0.986 atm
#b. He at 37.5 K and 7500 torr
Pressure, P = (7500 / 760) atm = 9.86 atm
#c. CH at 37.50C and 7.5 atm
Temperature, T = (37.5 + 273.15) K = 310.65 K
#d. Ne at 3750C and 0.75 atm
Temperature, T = (375 + 273.15) K = 648.15 K
#e. SF6 at -37.50C and 0.75 atm
Temperature, T = (-37.5 + 273.15) K = 235.65 K
# An ideal gas is characterized by constituting of point masses and absence of all type of intermolecular interactions. At higher temperature, the molecules have higher kinetics energy which predominates the intermolecular interactions. At lower pressure, the molecules lie apart from each other (compared to the same under higher pressure); so, intermolecular interactions is minimized. Therefore, a gas approaches to ideal behavior when temperature is higher and pressure is lower on a relative scale.
In the given list, Ne is at highest temperature and lowest pressure simultaneously. Therefore, Ne is most likely to behave as an ideal gas under given conditions.
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