Question

What is the density of chlorine gas (MM = 71.0glmol) at 1.50 atm and 25.0C

Answer 1

Answer: D=4.35g/L

Step-by-step explanation:

The formula for density is
`D=(M)/(V)`. M is mass in grams and V is volume in liters.

Since we are give pressure and temperature, we can use the ideal gas law to find moles/volume. FInding moles/volume would give us the base for density. All we would have to do is convert moles to grams.

Ideal Gas Law: PV=nRT

`(n)/(V) =(P)/(RT)`

`(n)/(V)=(1.50 atm)/((0.08206Latm/Kmol)(25+274.15K))`

`(n)/(V) =(0.061309mol)/(L)`

Now that we have moles, we can use molar mass of chlorine gas to find grams.

`0.061309mol*(71.0g)/(mol) =4.3529g`

With our grams, we can find our density.

`D=(4.3529g)/(L)`

We need correct significant figures so our density is:

`D=(4.35g)/(L)`