Got a tip for us?
Let us know
Become a MacRumors Supporter for $50/year with no ads, ability to filter front page stories, and private forums.
Chemistry help?
- Thread starter emt1
- Start date
- Sort by reaction score
Use the ideal gas law to get the total volume and then divide that by the constant ideal gas volume. Then you have the number of moles and go from there.
Ideal gas law is PV=nRT
First plug in numbers and solve for n to find out your total number of moles.
Seems to me like you might have too many unknowns to solve this, but assuming that we can use the molar volume of a gas for V then your molar mass should be 35.65249 g/mol which is pretty close to Chlorine.
The molar volume of a gas is 22.4 liters, so your equation would be:
(1.086 atm)(22.4L)/(0.0821 L*atm/mol*K)(229.9K)=n
n will be your number of moles which works out to be 1.289 mol.
you divide your given mass of 45.95 grams by the 1.29 mol to get a molar mass of 35.62 grams/mol. Chlorine (which is a gas at most temperatures) has a molar mass of 35.45 grams/mol.
But where I think this might all fall apart is that I believe that the stated temperature is just shy of Chlorine's vaporization point. So unless I'm mistaken, at that temperature and pressure, Chlorine should be a solid.
It's been like 3 years since I was in Gen Chem so you'll understand if I'm wrong here.
SLC
The molar volume of a gas is 22.4 liters, so your equation would be:
(1.086 atm)(22.4L)/(0.0821 L*atm/mol*K)(229.9K)=n
n will be your number of moles which works out to be 1.289 mol.
you divide your given mass of 45.95 grams by the 1.29 mol to get a molar mass of 35.62 grams/mol. Chlorine (which is a gas at most temperatures) has a molar mass of 35.45 grams/mol.
But where I think this might all fall apart is that I believe that the stated temperature is just shy of Chlorine's vaporization point. So unless I'm mistaken, at that temperature and pressure, Chlorine should be a solid.
It's been like 3 years since I was in Gen Chem so you'll understand if I'm wrong here.
SLC