R = 0.0821 L.atm/mol.°KSample ID: AMass of the emptyErlenmeyer flask +rubber band + foilPressureTemperature (°C)Temperature (°K)Mass of flask + vapor +rubber band + foilMass of vapor (grams)Volume of FlaskCalculated number ofmoles (n)Molar Mass (g/mol)Average Molar Mass(g/mol)n=107.2189I atm95°℃368.15⁰K108.2090.9829PVRTMMTrial 1=330ml 0.33 L1*0.330.0821*368.15m:0.010 met0.9820.010=98.29/moln=Trial 2107.2189I atm95.1°C368.25°k108.29691.0789PVMM.=103 g/mol330ml=0.33L1* 0.330.0821 368.25mn.:0.010 mol1.6780.010=107.89/mol 3. The molar mass value you calculated is only approximately the true molar mass of theunknown sample (the two values are not identical). Suggest one possible source ofexperimental error that may have resulted in the deviation of your calculatedvalue from the true value. (81

To identify the possible source of experimental error that might have resulted in the deviation of…

The molar mass value you calculated is only approximately the true molar mass of the unknown sample (the two values are not identical). Suggest one possible source of experimental error that may have resulted in the deviation of your calculated value from the true value. (

The molar mass value you calculated is only approximately the true molar mass of the unknown sample (the two values are not identical). Suggest one possible source of experimental error that may have resulted in the deviation of your calculated value from the true value. (

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter8: Chemical Composition

Section: Chapter Questions

Problem 111AP

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

R = 0.0821 L.atm/mol.°K
Sample ID: A
Mass of the empty
Erlenmeyer flask +
rubber band + foil
Pressure
Temperature (°C)
Temperature (°K)
Mass of flask + vapor +
rubber band + foil
Mass of vapor (grams)
Volume of Flask
Calculated number of
moles (n)
Molar Mass (g/mol)
Average Molar Mass
(g/mol)
n=
107.2189
I atm
95°℃
368.15⁰K
108.209
0.9829
PV
RT
MM
Trial 1
=
330ml 0.33 L
1*0.33
0.0821*368.15
m
:0.010 met
0.982
0.010
=
98.29/mol
n=
Trial 2
107.2189
I atm
95.1°C
368.25°k
108.2969
1.0789
PV
MM.
=
103 g/mol
330ml=0.33L
1* 0.33
0.0821 368.25
m
n
.:0.010 mol
1.678
0.010
=107.89/mol

3. The molar mass value you calculated is only approximately the true molar mass of the
unknown sample (the two values are not identical). Suggest one possible source of
experimental error that may have resulted in the deviation of your calculated
value from the true value. (
81

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