calculate the total pressure of amixture of 8g of oxygen and 4g of hydrogen confined in a vessel of 1 dm^3 at 27 degree Celcius

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Solution

Moles of O2 = 8/32= 1/4
Moles of H2 = 4/2= 2
Therefore Total moles of both gas(n) = 1/4 + 2 = 9/4
Given :
V = 1 dm3
T = 300 K
R = 0.083 bar dm3 K-1mole-1
PV=nRT
P = (9 x 0.083 x 300)/(4 x 1) = 56.025 bar

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Calculate the total pressure of a mixture of 8 g of oxygen and 4g of hydrogen confined in vessel of

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(R = 0.083 b a r d m^{3} k^{- 1} {m o l}^{- 1})

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Q. The Total pressure in a mixture of

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[Take

R = 0.083 {bar dm}^{3} K^{- 1} {mol}^{- 1}

]

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calculate the total pressure of amixture of 8g of oxygen and 4g of hydrogen confined in a vessel of 1 dm^3 at 27 degree Celcius

Moles of O2 = 8/32= 1/4 Moles of H2 = 4/2= 2 Therefore Total moles of both gas(n) = 1/4 + 2 = 9/4 Given : V = 1 dm3 T = 300 K R = 0.083 bar dm3 K-1mole-1 PV=nRT P = (9 x 0.083 x 300)/(4 x 1) = 56.025 bar

Moles of O2 = 8/32= 1/4
Moles of H2 = 4/2= 2
Therefore Total moles of both gas(n) = 1/4 + 2 = 9/4
Given :
V = 1 dm3
T = 300 K
R = 0.083 bar dm3 K-1mole-1
PV=nRT
P = (9 x 0.083 x 300)/(4 x 1) = 56.025 bar