Question

Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)? a. All of these samples will have the same pressure b. 15 g N2 c. 15 g Xe d. 15 g CO2 e. 15 g Ne BONUS A 1.0-L gas mixture at 298 K and 763.0 mmHg is isolated and found to contain the following gases with the indicated partial pressures: 586.0 mmHg nitrogen, 158.0 mmHg oxygen, and some argon. What is a) the partial pressure, b) the mole fraction, and c) the mass of argon?

          Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)?
a. All of these samples will have the same pressure
b. 15 g N2
c. 15 g Xe
d. 15 g CO2
e. 15 g Ne

BONUS
A 1.0-L gas mixture at 298 K and 763.0 mmHg is isolated and found to contain the following gases with the indicated partial pressures: 586.0 mmHg nitrogen, 158.0 mmHg oxygen, and some argon.
What is a) the partial pressure, b) the mole fraction, and c) the mass of argon?

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$Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)? a. All of these samples will have the same pressure b. 15 g N2 c. 15 g Xe d. 15 g CO2 e. 15 g Ne BONUS A 1.0-L gas mixture at 298 K and 763.0 mmHg is isolated and found to contain the following gases with the indicated partial pressures: 586.0 mmHg nitrogen, 158.0 mmHg oxygen, and some argon. What is a) the partial pressure, b) the mole fraction, and c) the mass of argon?$

Added by Brandon R.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Madhur L

03/24/2023

Step 1

QUESTION 10: To determine which sample will have the lowest pressure, we need to consider the number of moles of each gas, since pressure is directly proportional to the number of moles (according to the ideal gas law: PV = nRT). Show more…

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Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)? a. All of these samples will have the same pressure b. 15 g N2 c. 15 g Xe d. 15 g CO2 e. 15 g Ne BONUS A 1.0-L gas mixture at 298 K and 763.0 mmHg is isolated and found to contain the following gases with the indicated partial pressures: 586.0 mmHg nitrogen, 158.0 mmHg oxygen, and some argon. What is a) the partial pressure, b) the mole fraction, and c) the mass of argon?

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00:01 Hello students, in the first part of the question we have been asked about the lowest pressure of the gas when 15 gram each of the gas is present.

00:10 According to the ideal gas equation, pressure multiplied by volume is equal to nrt, the pressure of a gas would be equal to nrt divided by v.

00:24 As the pressure is directly proportional to the number of moles, the pressure would be equal to the energy.

00:30 Highest for the gas having the highest number of moles the number of moles are equal to the given mass divided by the molar mass of an entity the number of moles of di -nitrogen gas would be equal to the given mass which is 15 divided by its molar mass which is 28 grams the number of moles of di -nitrogen come out to be 0 .53 moles.

01:13 For xenon, the number of moles would be equal to 15 grams which is the given mass divided by its molar mass which is 130 grams.

01:23 The number of moles for xenon come out to be 0 .1 mole.

01:29 The number of moles of carbon dioxide would be equal to its given mass divided.

01:36 By its smaller mass which is 44 grams.

01:40 The number of moles of carbon dioxide come out to be 0 .3 moles.

01:47 The number of moles of neon would be equal to its given mass 15 grams divided by its smaller mass which is 20 grams.

01:56 The number of moles for neon come out to be 0 .75 mole.

02:03 As xenon has least number of moles, it will have the lowest value of pressure.

02:22 In the next part, we have been given a mixture which contain nitrogen, oxygen and argon.

02:28 The total pressure of the mixture is 763m .hg.

02:32 We have to calculate the partial pressure of argon.

02:35 The partial pressure of argon would be equal to the total pressure of the mixing...

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