Calculate the volume occupied by 1 mole of gas (any gas) at 1 atm and 0 degree C

Question

Calculate the volume occupied by 1 mole of gas (any gas) at 1 atm and 0 degree C (known as STP, standard temperature and pressure)? Show your work, Why is it that real gases do not behave as ideal gases at very low temperatures? The following errors in procedure will affect the experimental result. Explain how each action causes an incorrect result. Heating was stopped before all of the Equip in the flask has evaporated Water remained on the outside of the flask and on the fall when the final mass determined The volume of the flask was assumed to be 125 mL and not actually measured as directed in step 14 and 15 A student had an unknown liquid and determined its molar mass by collecting data described in this experiment Volume of the 125-mL Erlenmeyer flask, 130.3 mL Atmospheric pressure 727 torr using these data calculate the liquid's molar mass and identify the unknown from Table 12.1 Show all of your work.

Explanation / Answer

1) So we have the ideal gas equation

PV=nRT

They are asking us to calculated the volume.

V=nRT/P

we need R, and given the units of the pressure we choose R= 0.082 Latm/Kmol

and T= 273.15 K

V= 1mol *  0.082 Latm/Kmol * 273.15 K / 1 atm

V= 22.4 L

2. When know that the different between the real gas and the ideal gas is that we take into account the intermolecular forces between the molecules and we obtain two new factors that will be taken in account for every calculation.

At very low temperatures, the movement of the particles is almost cero, so all that intermolucar forces will not act between molecules. This is why the ideal gasses at low temperature behaves like ideal gasses.

3. a) If the heating stops before the complete evaporation the moles of gas will not be complete.

b) Any litlle change in the mass will count, so if you have some water that should not be taking into account, it will vaie the mass that you are meassuring.

c) Remember that the equation take into account the volume. So if you do some error doing the volume measuring when you do your calculations you will not have the exact number you are looking for. Always remember the measured all the volumes the most exactly you can!

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