if 16g of He is mixed with 32 g of O2 then calculate heat capacity ratio of the mixture
Answers
Given:
The mass of He = 16 g
The mass of O₂ = 32 g
To find:
The heat capacity ratio of the mixture
Solution:
Finding the no. of moles of bothe the gases:
The molar mass of He = 4 g/mol
The molar mass of O₂ = 32 g/mol
Let "n1" be the no. of moles of He and "n2" be the no. of moles of O₂
∴ n1 =
and
∴ n2 =
Finding the "" specific heat capacity at constant volume and "" specific heat capacity at constant pressure for the mixture:
Since
Helium is a mono-atomic gas ∴ γ₁ =
Oxygen is a diatomic gas ∴ γ₂ =
So,
The specific heat capacity at constant volume of He is,
= [R]/[γ₁ - 1] = [R] / [] = [R] / [] =
The specific heat capacity at constant volume of O₂ is,
= [R]/[γ₂ - 1] = [R] / [] = [R] / [] =
The specific heat capacity of the mixture at constant volume is given as,
The specific heat capacity of the mixture at constant pressure is given as,
Finding the ratio of the specific heat capacity of the mixture:
∴ The ratio of the specific heat capacity of the mixture,
γ_mix = =
Thus, the heat capacity ratio of the mixture is 27:17.
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The heat capacity ratio of the mixture is 27 : 17
Explanation:
The number of moles is given by the formula:
n = (Mass)/(Molar mass)
Now, the number of moles of helium:
n₁ = 16/4 = 4 moles
The number of moles of oxygen:
n₂ = 32/32 = 1 mole
The specific heat at constant volume is given by the formula:
Cv = R/(γ - 1)
The specific heat of helium at constant volume :
Cv₁ = R/(5/3 - 1) = 3R/2
The specific heat of oxygen at constant volume :
Cv₂ = R/(7/5 - 1) = 5R/2
The specific heat of mixture at constant volume is given as:
Cv = ((n₁ × Cv₁) + (n₂ × Cv₂))/(n₁ + n₂)
On substituting the values, we get,
Cv = ((4 × 3R/2) + (1 × 5R/2))/(4 + 1)
∴ Cv = 17R/10
The specific heat of mixture at constant pressure is given as:
Cp = Cv + R = 17R/10 + R
∴ Cp = 27R/10
The ratio of specific heat capacity of the mixture is given as:
γ = Cp/Cv
On substituting the values, we get,
γ = (17R/10)/(27R/10)
∴ γ = 27/17 = 27 : 17