Consider three gases: Ar, SF6, and Cl2. If 50.0 grams of these gases are placed in each of three identical containers, which container will have the highest pressure? The volume and temperature of all three containers are the same.
Answer (2)
To work this out we need to know that 1 mol of any gas will take up 24dm^3 of space at atmospheric pressure and temperature. Now we need to work out how many moles of each we have. To do this we also need to know the 1 mole is x grams of a chemical with molar mass of x Ar has a molar mass of 40 therefore 50 grams will be 1.25 moles SF6 has a molar mass of 146 therefore 50 grams will be approximatly 0.3 moles Cl2 has a molar mass of 71 therefore 50 grams will be approximately 0.7 moles Thus we can conclude that at atmospheric temperature and pressure the argon would take up the largest volume and thus when volume is limited it's pressure would be greatest
Argon (Ar) will have the highest pressure because it has the greatest number of moles (1.25 mol) compared to Sulfur Hexafluoride (SF6) and Chlorine (Cl2). The moles calculated for SF6 is approximately 0.343 mol and for Cl2 is approximately 0.704 mol. Therefore, with all conditions being equal, the pressure will be highest in the container with Argon.
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