Answer:
1.77 atm
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:
[tex]354.5g~\frac{1~mol}{70.9~g}[/tex]
[tex]5~mol[/tex]
Now, we have the moles, volume, temperature therefore we can use the ideal gas equation:
[tex]P*V=n*R*T[/tex]
We know the R value:
[tex]0.082\frac{atm*L}{mol*K}[/tex]
We have “K” units for the temperature, so we need to do the conversion:
[tex]30+273.15=303.15~K[/tex]
With all the data we can plug the values into the equation:
[tex]P*70L=5mol*303.15K*0.082\frac{atm*L}{mol*K} [/tex]
[tex]P=\frac{5mol*303.15K*0.082\frac{atm*L}{mol*K}}{70L}[/tex]
[tex]P=1.77~atm [/tex]
I hope it helps!
