Calculate the total pressure in a 10 litre cylinder which contains 0.4 g he, 1.6 g oxygen and 1.4 g nitrogen at 27°c. Also calculate the partial pressure of he gas in the cylinder. Assume ideal behavious for gases
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Answered by
67
PV = nRT V = 10 litre T = 27ºC = 300K
nHe = 0.4/4 = 0.1
N2 = 1.4/ 28= 0.05,
O2 = 1.6/32= 0.05
Total no. of moles = 0.1 + 0.05 + 0.05 0.2
PV = nRT P× 10 = 0.2 × 0.082 × 300 = 0.04926 P = 0.492 atm
Partial pressure = Total pressure × molefraction
PHe = 0.492 × 0.1/ 0.2
= 0.246 atm
PN2 = 0.492 × 0.05/ 0.2
= 0.123 atm
PO2 = 0.492 × 0.05/0.2
= 0.123 atm.
Mark Brian last
nHe = 0.4/4 = 0.1
N2 = 1.4/ 28= 0.05,
O2 = 1.6/32= 0.05
Total no. of moles = 0.1 + 0.05 + 0.05 0.2
PV = nRT P× 10 = 0.2 × 0.082 × 300 = 0.04926 P = 0.492 atm
Partial pressure = Total pressure × molefraction
PHe = 0.492 × 0.1/ 0.2
= 0.246 atm
PN2 = 0.492 × 0.05/ 0.2
= 0.123 atm
PO2 = 0.492 × 0.05/0.2
= 0.123 atm.
Mark Brian last
Answered by
7
Answer:
Moles of He = w/M = 0.4/4 = 0.10
Moles of O = w/M = 1.6/32 = 0.05 2
Moles of N = w/M = 1.4/28 = 0.05 2
Total moles = 0.2
PV = nRT
P x 10 = 0.2 x 0.082 x 300
P = 0.492 atm
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