If a gas in a closed container is pressurized from 14.9 atm to 16.5 atm and its original temperature was 33.1 °C, what would the
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<u>Answer:</u>
<u>For 1:</u> The partial pressure of helium is 376 mmHg and that of methane gas is 445 mmHg
<u>For 2:</u> The mole fraction of nitrogen gas is 0.392 and that of carbon dioxide gas is 0.608
<u>Explanation:</u>
<u>For 1:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For helium:</u>
Given mass of helium = 0.723 g
Molar mass of helium = 4 g/mol
Putting values in equation 1, we get:
- <u>For methane gas:</u>
Given mass of methane gas = 3.43 g
Molar mass of methane gas = 16 g/mol
Putting values in equation 1, we get:
To calculate the mole fraction , we use the equation:
.......(2)
To calculate the partial pressure of gas, we use the equation given by Raoult's law, which is:
......(3)
- <u>For Helium gas:</u>
We are given:
Putting values in equation 2, we get:
Calculating the partial pressure by using equation 3, we get:
Putting values in equation 3, we get:
- <u>For Methane gas:</u>
We are given:
Putting values in equation 2, we get:
Calculating the partial pressure by using equation 3, we get:
Putting values in equation 3, we get:
Hence, the partial pressure of helium is 376 mmHg and that of methane gas is 445 mmHg
- <u>For 2:</u>
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:
<u>For nitrogen gas:</u>
<u>For carbon dioxide gas:</u>
Hence, the mole fraction of nitrogen gas is 0.392 and that of carbon dioxide gas is 0.608