Question

If 3.67 g of CO₂ gas is introduced into an evacuated 2.50 L flask at 65∘C, what is the pressure inside the flask?

Answer 1

Answer: 0.926 atm

Step-by-step explanation:

We're given a mass of CO₂ in g, volume in L, and temperature in ⁰C, and looking for the pressure. We'll use the ideal gas law, PV = nRT, and R is the gas constant, and it's 0.08206 L x atm/K x mol⁻¹. n is the number of moles of the gas, and we can calculate the number of moles of CO₂ gas by converting the g of CO₂ gas to moles using its molar mass, 44.01g/mol.

3.67g CO₂(
`(1 mol CO2)/(44.01g CO2)`) = 0.0834 mol CO₂ = n

Next, we need to convert our temperature from ⁰C to K by adding 273.15:

65⁰C + 273.15 = 338.15K

Now, we plug in our known values, V, n, R, and T, into the equation:

P(2.50L) = (0.0834 mol CO₂)(
`(0.08206L*atm)/(K*mol^(-1))`)(338.15K)

Now, solve for P:

P(2.50L) = (0.0834 mol CO₂)(
`(0.08206L*atm)/(K*mol^(-1))`)(338.15K)
P(2.50L) = 2.314 L x atm
P =
`(2.314 L*atm)/(2.50L)`
= 0.926 atm

I hope this helps! :)