0.16 mol of argon gas is admitted to an evacuated 90 cm3 container at 30 ∘C. The gas then undergoes an isochoric heating to a temperature of 400 ∘C.
What is the final pressure of the gas?
Universal gas constant = R = 8.314 J/(K.mol)
Number of moles of the argon gas = n = 0.16 mol
Initial volume of the gas = V1 = 90 cm3 = 9 x 10-5 m3
Initial temperature of the gas = T1 = 30 oC = 303 K
Initial pressure of the gas = P1
Final volume of the gas = V2
Final temperature of the gas = T2 = 400 oC = 673 K
Final pressure of the gas = P2
The process is isochoric therefore,
V2 = V1 = 9 x 10-5 m3
P2V2 = nRT2
P2(9x10-5) = (0.16)(8.314)(673)
P2 = 9.947 x 106 Pa
Final pressure of the gas = 9.947 x 106 Pa
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