Using van der Waals equation determine the pressure exerted by 3.00 mol of Ar gas with a volume of 50.0 L at 25.0 °C.

Question

Question

in progress 0

Chemistry RI SƠ 1 year 2021-08-30T14:06:17+00:00 2021-08-30T14:06:17+00:00 1 Answers 10 views 0

Answers ( )

thuthuy · Answer 1 · 2021-08-30T14:07:55+00:00

Answer:

1.47 atm

Explanation:

From the question.

Applying

PV = nRT…………….. Equation 1

Where P = pressure, V = volume, T = temperature, n = number of moles, R = Molar gas constant

Makr P the subject of the equation

P = nRT/V……………. Euqation 2

Given: V = 50.0 L, n = 3.00 mol, T = 25°C = (273+25) = 298K,

Constant: R = 0.082 atm.L.K⁻¹mol⁻¹

Substitute these values into equation 2

P = (3×298×0.082)/(50)

P = 73.308/50

P = 1.46616

P ≈ 1.47 atm

Using van der Waals equation determine the pressure exerted by 3.00 mol of Ar gas with a volume of 50.0 L at 25.0 °C.​