A mixture of helium and methane gases, at a total pressure of 821 mm Hg, contains 0.723 grams of helium and 3.43 grams of methane. What is the partial pressure of each gas in the mixture?

PHe = mm Hg
PCH4 = mm Hg

2.) A mixture of nitrogen and carbon dioxide gases contains nitrogen at a partial pressure of 363 mm Hg and carbon dioxide at a partial pressure of 564 mm Hg. What is the mole fraction of each gas in the mixture?

XN2 =
XCO2 =

Question

06-12-2019
Chemistry

contestada

A mixture of helium and methane gases, at a total pressure of 821 mm Hg, contains 0.723 grams of helium and 3.43 grams of methane. What is the partial pressure of each gas in the mixture?

PHe = mm Hg
PCH4 = mm Hg

2.) A mixture of nitrogen and carbon dioxide gases contains nitrogen at a partial pressure of 363 mm Hg and carbon dioxide at a partial pressure of 564 mm Hg. What is the mole fraction of each gas in the mixture?

XN2 =
XCO2 =

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Аноним Аноним · Answer 1 · 2019-12-09T06:56:57+01:00

Answer:

For 1: The partial pressure of helium is 376 mmHg and that of methane gas is 445 mmHg

For 2: The mole fraction of nitrogen gas is 0.392 and that of carbon dioxide gas is 0.608

Explanation:

For 1:

To calculate the number of moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)

For helium:

Given mass of helium = 0.723 g

Molar mass of helium = 4 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of helium}=\frac{0.723g}{4g/mol}=0.181mol[/tex]

For methane gas:

Given mass of methane gas = 3.43 g

Molar mass of methane gas = 16 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of methane gas}=\frac{3.43g}{16g/mol}=0.214mol[/tex]

To calculate the mole fraction , we use the equation:

[tex]\chi_A=\frac{n_A}{n_A+n_B}[/tex] .......(2)

To calculate the partial pressure of gas, we use the equation given by Raoult's law, which is:

[tex]p_{A}=p_T\times \chi_{A}[/tex] ......(3)

For Helium gas:

We are given:

[tex]n_{He}=0.181mol\\n_{CH_4}=0.214mol[/tex]

Putting values in equation 2, we get:

[tex]\chi_{He}=\frac{0.181}{0.181+0.214}=0.458[/tex]

Calculating the partial pressure by using equation 3, we get:

[tex]p_T=821mmHg\\\\\chi_{He}=0.458[/tex]

Putting values in equation 3, we get:

[tex]p_{He}=0.458\times 821mmHg=376mmHg[/tex]

For Methane gas:

We are given:

[tex]n_{He}=0.181mol\\n_{CH_4}=0.214mol[/tex]

Putting values in equation 2, we get:

[tex]\chi_{CH_4}=\frac{0.214}{0.181+0.214}=0.542[/tex]

Calculating the partial pressure by using equation 3, we get:

[tex]p_T=821mmHg\\\\\chi_{CH_4}=0.542[/tex]

Putting values in equation 3, we get:

[tex]p_{CH_4}=0.542\times 821mmHg=445mmHg[/tex]

Hence, the partial pressure of helium is 376 mmHg and that of methane gas is 445 mmHg

For 2:

We are given:

Partial pressure of nitrogen gas = 363 mmHg

Partial pressure of carbon dioxide gas = 564 mmHg

Total pressure = (363 + 564) mmHg = 927 mmHg

Calculating the mole fraction of the gases by using equation 3:

For nitrogen gas:

[tex]363=\chi_{N_2}\times 927\\\\\chi_{N_2}=\frac{363}{927}=0.392[/tex]

For carbon dioxide gas:

[tex]564=\chi_{CO_2}\times 927\\\\\chi_{CO_2}=\frac{564}{927}=0.608[/tex]

Hence, the mole fraction of nitrogen gas is 0.392 and that of carbon dioxide gas is 0.608