Question

A gas mixture contains each of the following gases at the indicated partial pressures: N2, 211 torr ; O2, 141 torr ; and He, 159 torr .

**Part B**

What mass of each gas is present in a 1.15 −L sample of this mixture at 25.0 ∘C?

Answer #1

T = 25 0C

= 298 k

for N2

pN2 = 211 torr

= 0.278 atm

use,

p*v = n*R*T

0.278*1.15 = n*0.082*298

n = 0.0131 mole

(mass of N2)/ = 0.0131*(molar mass of N2)

molar mass of N2 = 28 g/mol

(mass of N2) = 0.0131*28

= 0.367 g

for O2

pO2 = 141 torr

= 0.186 atm

use,

p*v = n*R*T

0.187*1.15 = n*0.082*298

n = 8.8*10^-3 mole

(mass of O2) = 8.8*10^-3*(molar mass of N2)

molar mass of O2 = 32 g/mol

(mass of O2) = 8.8*10^-3*32

= 0.282 g

pHe = 159 torr

= 0.209 atm

use,

p*v = n*R*T

0.209*1.15 = n*0.082*298

n = 9.84*10^-3 mole

(mass of He) = 9.84*10^-3*(molar mass of N2)

molar mass of He = 4 g/mol

(mass of He) = 9.84*10^-3*4

= 0.0394 g

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indicated partial pressures: N2, 211 torr ; O2, 135 torr ; and He,
129 torr .
What mass of each gas is present in a 1.35 −L sample of this
mixture at 25.0 ∘C?

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indicated partial pressures: N2, 211 torr ; O2, 135 torr ; and He,
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1. What is the total pressure of the mixture?
2. What mass of each gas is present in a 1.35 −L sample of this
mixture at 25.0 ∘C?

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B.) What mass of each gas is present in a 1.25 −L sample of this
mixture at 25.0 ∘C?
mN2, mO2, mHe =

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