Question

354.5 g of chlorine gas (MW = 70.9 g/mol) is held in a vessel with a fixed volume of 70. L.

What is the pressure of the gas in atmospheres if it's temperature is 30.0°C?


___ atm

Answer 1

1.77 atm

Step-by-step explanation:

We have to check the values that gives the problem:

V= 70 L

mass =354.5 g

Molas weight= 70.9 g/mol

T=30 ºC

P= ?

We can find the moles of chlorine if we use the molar weight:

`354.5g~(1~mol)/(70.9~g)`

`5~mol`

Now, we have the moles, volume, temperature therefore we can use the ideal gas equation:

`P*V=n*R*T`

We know the R value:

`0.082(atm*L)/(mol*K)`

We have “K” units for the temperature, so we need to do the conversion:

`30+273.15=303.15~K`

With all the data we can plug the values into the equation:

`P*70L=5mol*303.15K*0.082(atm*L)/(mol*K)`

`P=(5mol*303.15K*0.082(atm*L)/(mol*K))/(70L)`

`P=1.77~atm`

I hope it helps!