Answer:
the pressure is P = 5,94 atm ≈ 6 atm
Explanation:
Following the equation corresponding to the Ideal Gas Law, it is possible to find the system pressure in the silver problem.
[tex]PV = nRT[/tex]
From this equation, we find the pressure
[tex]P = \frac{nRT}{V}[/tex]
where:
P is the pressure of the gas,
V is the volume of the gas,
n is the amount of substance of gas (also known as number of moles),
R is the ideal, or universal, gas constant.
Now we find the moles of CO2
[tex]n = \frac{g}{PM}[/tex]
We have 375g of CO2 and its molecular weight is 44g/mol
[tex]nCO_{2} = \frac{375g}{44g/mol} = 8,52 mol[/tex]
Using.
R = 0,082[tex]\frac{L . atm}{K . mol}[/tex]
T = 20ºC = 293,15 K
We substitute in the equation
[tex]P = \frac{nRT}{V}\\\\ P = \frac{8,52 mol . 0,082\frac{L.atm}{K . mol} . 293,15K}{34,5 L}\\[/tex]
P = 5,94 atm ≈ 6 atm
