GUYS this is URGENT?

Question

Ok, I seriously need this ASAP.

the question says, The density of methanol is 0.796 g/cm3. Is 4.00 mL of methanol a satisfactory volume to use in this experiment? Justify your answer with a calculation.

THe only thing I have for methanol is its molecular weight, 49.28 g/mol.

But I dont have the temperature of the REQUIRED moles of methanol!!! how am i supposed to do this??? This is what I did:

Since, density = mass/volume
0.796g/cm3 = mass / 4cm3
Mass= 3.184 g

Further, number of moles = mass / molar mass
n = 3.184 g / 49.28 g/mol
n= 0.06448 mols

To find the required number of moles, we use the ideal gas law:
PV = nRT
n = PV/RT (T ???)
n =

and what about the volume?? All i know is that the molecular weight of the IDEAL/ required methanol is 32.04 g/mol

HELP ME FOLKS PLEASEEE QUICK. THANKSSS

I am using the ideal gas law because we've added the methanol into a flask and put it in a hot water boiling bath, which makes it vaporize, then after cooling, it condenses into liquid and we can weigh it and calculate its molecular weight USING the gas law.

Answer 1

It's hard to answer this without knowing what experiment you are doing! If you are trying to make methanol vapor fill a certian size volume container and you need to know if 4 g will form enough vapor? I would set pressure to 1 ATM and temp to the boiling point of methanol (65 C); you already have n:

V = nRT/P remember: V in liters, P in ATM; T in Kelvin!

V = [0.0645mol x 0.08206latm/molK x (273 + 65)]/1 ATM =

V = 1.79 liters

I have no idea if this is what you are looking for.

Added: OK; now I know what you're trying to do!

Do the calculation I just did, but use the temperature of 100C (373 K) in the equation instead of 65 C. Then, see if the volume of vapor produced is larger than the container you were filling. Generally, when doing these experiments the container has a small vent so the pressure stays at 1 ATM and any extra gas just escapes. So the weight of the condensed liquid is the same as the weight of vapor that just filled the container under the conditions of T and P that were in effect when the container was full of the vapor.

Answer 2

The Methanol is liquid. Why are you using the ideal gas law?

Your question is:

"the question says, The density of methanol is 0.796 g/cm3. Is 4.00 mL of methanol a satisfactory volume to use in this experiment?"

In what experiment? What reaction are we doing with the methanol?

Aha! a dumas bulb. The volume of the bulb is probably somewhere between 25 -100ml. If you solve the volume of your 0.06448 moles of Methanol at 100 C.you will find that it is at least 1.5 liter of vapor. So that is plenty to fill the little dumas bulb with vapor.

Answer 3

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