What mass, in grams, of chlorine gas (Cl2) is contained in a 12.5 liter tank at 27.0 degrees Celsius and 2.85 atmospheres? Show all of the work used to solve this problem.
Please explain step by step how to solve this so I can study it for the test. I just do not understand it. Thanks.
Please explain step by step how to solve this so I can study it for the test. I just do not understand it. Thanks.
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You're given:
- Volume
- Temperature
- Pressure
You're required to find the mass.
Any equation comes to mind? Remember, you can find mass from moles and moles from mass!
pV= nRT
So let's find 'n':
n = pV/RT
n = (2.85 atm) (12.5 L) / (0.08206 L atm / K mol) (27 + 273 K)
n = 1.45 mol
Now we know that: Atomic Mass of Cl2 = 35.5 x2 = 71 g/mol
So we can calculate the mass!
Number of moles = mass/atomic mass
mass = number of moles x atomic mass
mass = n x 71 g/mol
mass = 1.45 mol x 71 g/mol
mass = 102.74 g
And that's it! Easy wasn't it? :)
- Volume
- Temperature
- Pressure
You're required to find the mass.
Any equation comes to mind? Remember, you can find mass from moles and moles from mass!
pV= nRT
So let's find 'n':
n = pV/RT
n = (2.85 atm) (12.5 L) / (0.08206 L atm / K mol) (27 + 273 K)
n = 1.45 mol
Now we know that: Atomic Mass of Cl2 = 35.5 x2 = 71 g/mol
So we can calculate the mass!
Number of moles = mass/atomic mass
mass = number of moles x atomic mass
mass = n x 71 g/mol
mass = 1.45 mol x 71 g/mol
mass = 102.74 g
And that's it! Easy wasn't it? :)