A 8.15-L container holds a mixture of two gases at 31 °C. The partial pressures of gas A and gas B, respectively, are 0.215 atm and 0.833 atm. If 0.160 mol of a third gas is added with no change in volume or temperature, what will the total pressure become? In atm
total pressure initially = sum of partial pressure of A and B = 0.215 atm + 0.813 atm = 1.028 atm
PV = nRT
P = 1.028 atm
V = 8.15 L
n = ? mol
R = gas constant = 0.082057 Latmmol^-1K^-1
T = temp in Kelvin = 273 +31 = 304 K
1.028 x 8.15 = n x 0.0821 x 304
8.3782 = n x 24.95
n = 8.3782 / 24.95
n = 0.336 moles
there are the moles of gas initially
now new moles = 0.336 + 0.160 = 0.5 moles
again
P = ? atm
V = 8.15 L
n = 0.5 mol
R = 0.082057 Latmmol^-1K^-1
T = 304 K
P x 8.15 = 0.5 x 0.0821 x 304
P = 12.5/8.15
P = 1.5. atm
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