Question

A mixture of 0.220 moles co, 0.350 moles f2 and 0.640 moles he has a total pressure of 2.95 atm. what is the pressure of co?

Answer 1

The pressure of CO is $\boxed{{\text{0}}{\text{.536 atm}}}$  .

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, ${{\text{F}}_2}$  and He. The expression to calculate partial pressure of CO is,

${P_{{\text{CO}}}} = {X_{{\text{CO}}}}\cdot {P_{{\text{total}}}}$                                                                        ….. (1)

Here,

${P_{{\text{CO}}}}$ is the partial pressure of CO.

${P_{{\text{total}}}}$ is the total pressure of the mixture.

${X_{{\text{CO}}}}$ is the mole fraction of CO.

The mole fraction of CO is calculated as follows:

${X_{{\text{CO}}}} = \frac{{{\text{Number of moles of CO}}}}{{{\text{Total number of moles}}}}$                                             …… (2)

The formula to calculate total number of moles in the mixture is as follows:

${\text{Total number of moles}}={\text{Moles of}}\;{\text{CO}}+{\text{Moles of }}{{\text{F}}_2}+{\text{Moles}}\;{\text{of}}\;{\text{He}}$            …… (3)

Substitute 0.220 mol for the moles of CO, 0.350 mol for the moles of ${{\text{F}}_2}$  and 0.640 mol for the moles of He in equation (3).

$\begin{aligned}{\text{Total number of moles}}&={\text{0}}{\text{.220 mol}}+{\text{0}}{\text{.350 mol}}+{\text{0}}{\text{.640 mol}}\\&={\text{1}}{\text{.21 mol}}\\\end{aligned}$

Substitute 0.220 mol for the moles of CO and 1.21 mol for the total number of moles in equation (2).

$\begin{aligned}{X_{{\text{CO}}}}&=\frac{{{\text{0}}{\text{.220 mol}}}}{{{\text{1}}{\text{.21 mol}}}}\\&= 0.1818\\\end{aligned}$

The value of ${X_{{\text{CO}}}}$  is 0.1818.

The value of ${P_{{\text{total}}}}$  is 2.95 atm.

Substitute these values in equation (1).

$\begin{aligned}{P_{{\text{CO}}}}&=\left({0.1818}\right)\left({{\text{2}}{\text{.95 atm}}}\right)\\&=0.{\text{53631 atm}}\\&\approx0.{\text{536 atm}}\\\end{aligned}$

So the partial pressure of CO is 0.536 atm.

Learn more:

1. Calculate the moles of chlorine in 8 moles of carbon tetrachloride: brainly.com/question/3064603

2. Which law states the direct relationship between volume and absolute temperature at constant pressure? 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.

Answer 2

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:

$P_{total} \ = P_{1} + P_2 + P_3+...P_n$

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:

$P_x = P_{total} \times \frac{n_x}{n_total}$

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:

$P_{CO} = 2.95 \ atm \times \frac{0.220 mol CO}{1.21 \ mol}\\\\\boxed {\boxed {P_{CO} = 0.536 \ atm}}}$

Learn More

1. Ideal Gas Law brainly.com/question/12936013
2. Root Mean Square brainly.com/question/5980325

Keywords: Dalton's Law of Partial Pressure, mole ratio