If 0.750 L of argon at 1.50 atm and 177oC and 0.235 L of sulfur dioxide at 95.0 kPa and 63.0oC are added to a 1.00 L flask and the flask's temperature is adjusted to 25.0oC

Question

what is the resulting pressure in the flask?

0.0851 atm

0.244 atm

1.74 atm

0.946 atm

Answer 1

Find number of moles for: If 0.750 L of argon at 1.50 atm and 177^oC...

P V = n R T

(1.50) (0.750) = n (0.08206) (443.15)

1.125 = n (36.36)

1.125 / 36.36 = n

0.031 mol Ar = n

Find number of moles for: 0.235 L of sulfur dioxide at 95.0 kPa and 63.0^oC...

Convert kPa to atm conversion: 95.0 kPa x (1 atm / 101.325 kPa) = 0.94 atm

P V = n R T

(0.94) (0.235) = n (0.08206) (336.15)

0.2209 = n (27.58)

0.2209 / 27.58 = n

0.008 mol SO₂ = n

Add up the moles to get the total moles in the mixture, then use the information for the final mixture to solve for the pressure of the final mixture:

0.031 mol Ar + 0.008 mol SO₂ = 0.039 total mol

P V = n R T

P (1) = (0.039) (0.08206) (298.15)

P (1) = 0.9542

P = 0.9542 / 1

P = 0.94 atm

Answer: D (0.946 atm)