ALEKS 360-ACCESS (52 WEEKS)
ALEKS 360-ACCESS (52 WEEKS)
4th Edition
ISBN: 9781260996760
Author: Burdge
Publisher: MCG
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Textbook Question
Chapter 10, Problem 1KSP

Determine the mole fraction of helium in a gaseous mixture consisting of 0.524 g He, 0 .275 g Ar . and 2 .05 g C H 4 .

(a)

0.0069

(b)

0.0259

(c)

0.481

(d)

0.493

(e)

0.131

Expert Solution & Answer
Check Mark
Interpretation Introduction

Interpretation:

The mole fraction of helium in a gaseous mixture is to be calculated.

Concept introduction:

The mole fraction of an individual gas, for a combination of gases, is the ratio of the moles of the individual gas to the total number of moles of the mixture.

χi=nintotal

Here, χi is the mole fraction, ni is the mole fraction of individual gas, and ntotal is the total number of moles.

Also, the mole fraction of an individual gas, for a combination of gases, can be calculated from the ratio of the partial pressure of the individual gas to the total pressure of the combination.

χi=PiPtotal

Here, χi is the mole fraction, Pi is the partial pressure of individual gas, and Ptotal is the total pressure.

The number of moles can be calculated as

n=mM

Here, m represents the mass of the molecule, M represents the molar mass of the molecule, and n is the number of moles.

Answer to Problem 1KSP

Solution: Option (d).

Explanation of Solution

Given information:

Mass of helium mHe=0.524 g

Mass of argon mAr=0.275 g

Mass of methane mCH4=2.05 g

Reason for the correct option:

The molar mass of helium is 4 g/mol.

Calculate the number of moles of helium as follows:

nHe=mHeMHe

Substitute 0.524 g for nHe and 4 g/mol for MHe in the above equation

nHe=0.524 g4 g/mol=0.131 mol

The molar mass of argon is 39.9 g/mol.

Calculate the number of moles of argon as follows:

nAr=mArMAr

Substitute 0.275 g for nAr and 39.9 g/mol for MAr in the above equation

nAr=0.275 g39.9 g/mol=0.0069 mol

The molar mass of methane is 16 g/mol.

Calculate the number of moles of methane as follows:

nCH4=mCH4MCH4

Substitute 2.05 g for nCH4 and 16 g/mol for MCH4 in the above equation

nCH4=2.05 g16 g/mol=0.128 mol

From Dalton’s law for the combination of gases, the total number of moles can be calculated as

ntotal=ni=nHe+nAr+nCH4

Substitute 0.0069 mol for nAr, 0.128 mol for nCH4, and 0.131 mol for nHe in the above equation

ntotal=0.131 mol+0.0069 mol+0.128 mol=0.266 mol

Calculate the mole fraction for He gas as follows:

χHe=nHentotal

Substitute 0.266 mol for ntotal and 0.131 mol for nHe in the above equation

χHe=0.131 mol mol0.266 mol mol=0.493

Thus, for He, the mole fraction is 0.493.

Hence, option (d) is correct.

Reason for the incorrect options:

Option (a) is incorrect because the calculated value of mole fraction of heliumfor the given gaseous mixturedoes not match the given value in option (a).

Option (b) is incorrect because the calculated value of mole fraction of helium for the given gaseous mixturedoes not match the given value in option (b).

Option (c) is incorrect because the calculated value of mole fraction of helium for the given gaseous mixturedoes not match the given value in option (c).

Option (e) is incorrect because the calculated value of mole fraction of helium for the given gaseous mixturedoes not match the given value in option (e).

Hence, options(a), (b), (c), and (e) are incorrect.

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Chapter 10 Solutions

ALEKS 360-ACCESS (52 WEEKS)

Ch. 10.2 - Prob. 1PPCCh. 10.2 - 10.2.1 Given . Ch. 10.2 - Prob. 2CPCh. 10.2 - 10.2.3 At what temperature will a gas sample...Ch. 10.2 - What volume of NH 3 will be produced when 180 mL...Ch. 10.2 - Prob. 5CPCh. 10.2 - Prob. 6CPCh. 10.3 - Practice ProblemATTEMPT A sample of gas originally...Ch. 10.3 - Practice ProblemBUILD At what temperature (in °C )...Ch. 10.3 - Prob. 1PPCCh. 10.3 - Prob. 1CPCh. 10.3 - Prob. 2CPCh. 10.3 - Prob. 3CPCh. 10.3 - Prob. 4CPCh. 10.4 - Practice ProblemATTEMPT What volume (in liters) of...Ch. 10.4 - Practice ProblemBUILD What volumes (in liters) of...Ch. 10.4 - Practice Problem CONCEPTUALIZE A hypothetical...Ch. 10.4 - Prob. 1CPCh. 10.4 - Prob. 2CPCh. 10.5 - Practice Problem ATTEMPT What would be the volume...Ch. 10.5 - Prob. 1PPBCh. 10.5 - Prob. 1PPCCh. 10.5 - Prob. 1CPCh. 10.5 - Prob. 2CPCh. 10.5 - Prob. 3CPCh. 10.5 - 10.5.4 What mass of acetylene is produced by the...Ch. 10.5 - In the following diagram, each color represents a...Ch. 10.5 - Prob. 6CPCh. 10.6 - Practice ProblemATTEMPT What is the volume of 5.12...Ch. 10.6 - Practice ProblemBUILD At what temperature ( in °C...Ch. 10.6 - Practice Problem CONCEPTUALIZE The diagram shown...Ch. 10.6 - Prob. 1CPCh. 10.6 - Prob. 2CPCh. 10.7 - Practice Problem ATTEMPT Calculate the density of...Ch. 10.7 - Prob. 1PPBCh. 10.7 - Prob. 1PPCCh. 10.7 - Prob. 1CPCh. 10.7 - Prob. 2CPCh. 10.8 - Practice Problem ATTEMPT Determine the molar mass...Ch. 10.8 - Practice Problem BUILD A sample of the volatile...Ch. 10.8 - Practice ProblemCONCEPTUALIZE These models...Ch. 10.9 - Practice Problem ATTEMPT What volume (in liters)...Ch. 10.9 - Practice Problem BUILD What mass (in grams) of Na...Ch. 10.9 - Prob. 1PPCCh. 10.10 - Practice Problem ATTEMPT Using all the same...Ch. 10.10 - Practice ProblemBUILD By how much would the...Ch. 10.10 - Prob. 1PPCCh. 10.11 - Prob. 1PPACh. 10.11 - Prob. 1PPBCh. 10.11 - Prob. 1PPCCh. 10.12 - Practice Problem ATTEMPT Determine the partial...Ch. 10.12 - Practice Problem BUILD Determine the number of...Ch. 10.12 - Prob. 1PPCCh. 10.13 - Prob. 1PPACh. 10.13 - Practice ProblemBUILD Determine the partial...Ch. 10.13 - Prob. 1PPCCh. 10.14 - Practice Problem ATTEMPT Calculate the mass of ...Ch. 10.14 - Practice ProblemBUILD Determine the volume of gas...Ch. 10.14 - Practice ProblemCONCEPTUALIZE The first diagram...Ch. 10.15 - Prob. 1PPACh. 10.15 - Practice ProblemBUILD What chamber pressure would...Ch. 10.15 - Practice ProblemCONCEPTUALIZE The diagram on the...Ch. 10.16 - Prob. 1PPACh. 10.16 - Practice ProblemBUILD Determine the molar mass and...Ch. 10.16 - Practice ProblemCONCEPTUALIZE The diagram on the...Ch. 10.17 - Practice ProblemATTEMPT Using data from Table...Ch. 10.17 - Practice ProblemBUILD Calculate the pressure...Ch. 10.17 - Practice ProblemCONCEPTUALIZE What properties of...Ch. 10 - Determine the mole fraction of helium in a gaseous...Ch. 10 - Prob. 2KSPCh. 10 - Determine the mole fraction of water in a solution...Ch. 10 - Prob. 4KSPCh. 10 - Prob. 1QPCh. 10 - Prob. 2QPCh. 10 - Prob. 3QPCh. 10 - Prob. 4QPCh. 10 - Prob. 5QPCh. 10 - Prob. 6QPCh. 10 - Prob. 7QPCh. 10 - Prob. 8QPCh. 10 - Prob. 9QPCh. 10 - Prob. 10QPCh. 10 - Prob. 11QPCh. 10 - Prob. 12QPCh. 10 - Prob. 13QPCh. 10 - Prob. 14QPCh. 10 - Calculate the height of a column of methanol (C H...Ch. 10 - Prob. 16QPCh. 10 - What pressure (in atm) is exerted by a column of...Ch. 10 - What pressure (in atm) is exerted by a column of...Ch. 10 - Prob. 19QPCh. 10 - Prob. 20QPCh. 10 - Prob. 21QPCh. 10 - Prob. 22QPCh. 10 - Prob. 23QPCh. 10 - A sample of air occupies 3.8 L when the pressure...Ch. 10 - Prob. 25QPCh. 10 - 10.26 Under constant-pressure conditions a sample...Ch. 10 - 10.27 Ammonia bums in oxygen gas to form nitric...Ch. 10 - Molecular chlorine and molecular fluorine combine...Ch. 10 - A gaseous sample of a substance is cooled at...Ch. 10 - Consider the following gaseous sample in a...Ch. 10 - Prob. 31QPCh. 10 - Prob. 32QPCh. 10 - Prob. 33QPCh. 10 - Prob. 34QPCh. 10 - 10.35 Given that 6.9 moles of carbon monoxide gas...Ch. 10 - What volume will 9.8 moles of sulfur hexafluoride...Ch. 10 - Prob. 37QPCh. 10 - Prob. 38QPCh. 10 - Prob. 39QPCh. 10 - An ideal gas originally at 0.85 atm and 66°C was...Ch. 10 - Calculate the volume (in liters) of 124.3 g of CO...Ch. 10 - Prob. 42QPCh. 10 - Prob. 43QPCh. 10 - Prob. 44QPCh. 10 - At 741 torr and 44°C, 7.10 g of a gas occupies a...Ch. 10 - Prob. 46QPCh. 10 - Assuming that air contains 78 percent N 2 , 21...Ch. 10 - 10.48 A 2.10-L vessel contains 4.65 g of a gas at...Ch. 10 - Calculate the density of hydrogen bromide ( HBr )...Ch. 10 - A certain anesthetic contains 64.9 percent C, 13.5...Ch. 10 - A compound has the empirical formula SF 4 . 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