Respuesta :
The partial pressure of CO is 0.536 atom.
Further Explanation
Dalton's Law of Partial Pressure states that the total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases. Mathematically, it can be represented as follows:
[tex]P_{total} \ = P_{1} + P_2 + P_3+...P_n[/tex]
If the total pressure is known as well as the number of moles of the gases in the mixture, the partial pressure of a component as can be calculated using the equation below:
[tex]P_x = P_{total} \times \frac{n_x}{n_total}[/tex]
where:
Pₓ is the partial pressure of gas X
P(total) = total pressure of the mixture
nₓ = number of moles of gas X
n(total) = total number of moles of gas
To solve the problem, first sort the given:
- n(total) = 0.220 mol CO + 0.350 mol F₂ + 0.640 mol He = 1.21 moles
- n(CO) = 0.220 mol
- P(total) = 2.95 atm
Then we plug in the given values into the equation above:
[tex]P_{CO} = 2.95 \ atm \times \frac{0.220 mol CO}{1.21 \ mol}\\\\\boxed {\boxed {P_{CO} = 0.536 \ atm}}}[/tex]
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Keywords: Dalton's Law of Partial Pressure, mole ratio
The pressure of CO is [tex]\boxed{{\text{0}}{\text{.536 atm}}}[/tex] .
Further explanation:
Dalton’s law:
According to this law, the total pressure of the gaseous mixture is the sum of partial pressure of each gas. The given mixture contains CO, [tex]{{\text{F}}_2}[/tex] and He. The expression to calculate partial pressure of CO is,
[tex]{P_{{\text{CO}}}} = {X_{{\text{CO}}}}\cdot {P_{{\text{total}}}}[/tex] ….. (1)
Here,
[tex]{P_{{\text{CO}}}}[/tex] is the partial pressure of CO.
[tex]{P_{{\text{total}}}}[/tex] is the total pressure of the mixture.
[tex]{X_{{\text{CO}}}}[/tex] is the mole fraction of CO.
The mole fraction of CO is calculated as follows:
[tex]{X_{{\text{CO}}}} = \frac{{{\text{Number of moles of CO}}}}{{{\text{Total number of moles}}}}[/tex] …… (2)
The formula to calculate total number of moles in the mixture is as follows:
[tex]{\text{Total number of moles}}={\text{Moles of}}\;{\text{CO}}+{\text{Moles of }}{{\text{F}}_2}+{\text{Moles}}\;{\text{of}}\;{\text{He}}[/tex] …… (3)
Substitute 0.220 mol for the moles of CO, 0.350 mol for the moles of [tex]{{\text{F}}_2}[/tex] and 0.640 mol for the moles of He in equation (3).
[tex]\begin{aligned}{\text{Total number of moles}}&={\text{0}}{\text{.220 mol}}+{\text{0}}{\text{.350 mol}}+{\text{0}}{\text{.640 mol}}\\&={\text{1}}{\text{.21 mol}}\\\end{aligned}[/tex]
Substitute 0.220 mol for the moles of CO and 1.21 mol for the total number of moles in equation (2).
[tex]\begin{aligned}{X_{{\text{CO}}}}&=\frac{{{\text{0}}{\text{.220 mol}}}}{{{\text{1}}{\text{.21 mol}}}}\\&= 0.1818\\\end{aligned}[/tex]
The value of [tex]{X_{{\text{CO}}}}[/tex] is 0.1818.
The value of [tex]{P_{{\text{total}}}}[/tex] is 2.95 atm.
Substitute these values in equation (1).
[tex]\begin{aligned}{P_{{\text{CO}}}}&=\left({0.1818}\right)\left({{\text{2}}{\text{.95 atm}}}\right)\\&=0.{\text{53631 atm}}\\&\approx0.{\text{536 atm}}\\\end{aligned}[/tex]
So the partial pressure of CO is 0.536 atm.
Learn more:
1. Calculate the moles of chlorine in 8 moles of carbon tetrachloride: https://brainly.com/question/3064603
2. Which law states the direct relationship between volume and absolute temperature at constant pressure? https://brainly.com/question/1403211
Answer details:
Grade: Middle School
Subject: Chemistry
Chapter: Gases and the kinetic-molecular theory
Keywords: moles, pressure, 0.220 mol, 0.640 mol, 0.0350 mol, 0.536 atm, 2.95 atm, He, CO, F2, moles of CO, moles of F2, moles of He, Dalton law and pressure of CO.
