At STP, 3L of chlorne is produced during a chemical reaction . What is the mass of this gas?

Answer 1

Ok, in order to solve this equation, you must use PV=nRT
At ATP:
P=1atm
V=3L CL2gas
n= what you are solving for
T=273K
R=.0821 Universal gas constant

Now just plug into the equation
(1)(3)=n(.0821)(273K)
n=.1339 Moles of CL2 gas
The molar mass of Cl2 gas is 71.0 grams/mol

Now just take 71.0 x .1339 and you get 9.5 grams.
I hope I helped thanks

I am 100% sure that this answer is correct.

Answer 2

1 mole of any ideal gas at STP is 22.4 Liters. Chlorine gas is close enough to an ideal gas to use that value. So divide to calculate the number of moles.

Remember that chlorine gas is diatomic, so use Cl2 to calculate the molar mass.

Once you have the number of moles and the molar mass, the rest is pretty easy.

Answer 3

the relevant equation is molar mass=gramsxRxT over PxV

chlorine weighs 70. and STP means 1atm and 273K. so:

70=g(0.0821)(273)
......____________
........(1)(3)

210=22.4133g

0.106 = g

therefore the gas weighed 0.106g

Note: "2 meter" gave an alternate solution, but this is easier.

Answer 4

At STP T=273K p=1 atm

pV = nRT

n= pV / RT = 1 ( 3 ) / 0.08296 (273) = 0.134 mole

MM (Cl2) = 70.906 g /mol

mass Cl2 = 0.134 ( 70.906 ) = 9.50g