DATA TABLE 2mL Mass of Erlenmeyer flask, rubber band and foil cover (g) Temperature of water bath (°C) Mass of Erlenmeyer flask, rubber band, foil cover and condensed gas sample (g) Mass of the condensed gas sample (g) Barometric (atmospheric) pressure (mmHg) Volume of the Erlenmeyer flask (mL) Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): of a column pressure of mercury to o certain height P = pressure (mmHg) DATA ANALYSIS (Show your calculations) 1. Determine the mass of the condensed portion of the unknown that you placed in the Erlenmeyer flask. me molar mass of the unknown sample can be calculated using the ideal gas law: #of mol я тетр (Equation 1) PV = nRT n= Trial 2 96.649 96.75 97°C 98°C 97.179 96.95 0.53g 0.20 762.18 762.18 152 mL 152mb ↓ idéal gos constant V = volume (mL) Trial 1 1 . Use the equation 4, along with the recorded temperature of the boiling water bath and the arometric (atmospheric) pressure of the room, to calculate the molar mass of your unknown Compound. R = 62,400- mL x mm Hg mol x °K ideal gas constant e number of moles, n, is the mass, in g, divided by the molar mass (M): m (g) M (g/mol) P= 30.03 (Equation 2) inches of column n = number of moles this is the only constant } mercury} We W m 30.03 Hg C
DATA TABLE 2mL Mass of Erlenmeyer flask, rubber band and foil cover (g) Temperature of water bath (°C) Mass of Erlenmeyer flask, rubber band, foil cover and condensed gas sample (g) Mass of the condensed gas sample (g) Barometric (atmospheric) pressure (mmHg) Volume of the Erlenmeyer flask (mL) Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): of a column pressure of mercury to o certain height P = pressure (mmHg) DATA ANALYSIS (Show your calculations) 1. Determine the mass of the condensed portion of the unknown that you placed in the Erlenmeyer flask. me molar mass of the unknown sample can be calculated using the ideal gas law: #of mol я тетр (Equation 1) PV = nRT n= Trial 2 96.649 96.75 97°C 98°C 97.179 96.95 0.53g 0.20 762.18 762.18 152 mL 152mb ↓ idéal gos constant V = volume (mL) Trial 1 1 . Use the equation 4, along with the recorded temperature of the boiling water bath and the arometric (atmospheric) pressure of the room, to calculate the molar mass of your unknown Compound. R = 62,400- mL x mm Hg mol x °K ideal gas constant e number of moles, n, is the mass, in g, divided by the molar mass (M): m (g) M (g/mol) P= 30.03 (Equation 2) inches of column n = number of moles this is the only constant } mercury} We W m 30.03 Hg C
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
Question
Transcribed Image Text:DATA TABLE
2mL
Mass of Erlenmeyer flask, rubber band and foil cover (g)
Temperature of water bath (°C)
Mass of Erlenmeyer flask, rubber band, foil cover and condensed
gas sample (g)
Mass of the condensed gas sample (g)
Barometric (atmospheric) pressure (mmHg)
Volume of the Erlenmeyer flask (mL)
Molar mass of the unknown sample (g/mole)
Average molar mass (g/mol):
of a column
9
pressure
of mercury to a
certain height
ideal gas constant
P = pressure (mmHg)
V = volume (mL)
R = 62,400
mL x mm Hg
mol x °K
ideal
gas constant
The number of moles, n, is the mass, in g, divided by the molar mass (M):
n
DATA ANALYSIS (Show your calculations)
1. Determine the mass of the condensed portion of the unknown that you placed in the
Erlenmeyer flask.
2. Use the equation 4, along with the recorded temperature of the boiling water bath and the
barometric (atmospheric) pressure of the room, to calculate the molar mass of your unknown
compound.
The molar mass of the unknown sample can be calculated using the ideal gas law:
# of mol
↑
PV = nRT
7
(Equation 1)
Temp
m (g)
M (g/mol)
aug.
Trial 1
Trial 2
96.649 96.75
97°C 98°C
97.179 96.95
0.53g 0.20
762.18 762.18
152 mL 152mL
(Equation 2)
P= 30.03
inches of mercury?
mercury?
column
n = number of moles
this is
the only
constant
}
we need
mm of
mercury
column
30.03
Hg
3
Imm=, 0394
Imm
.03 94N
Transcribed Image Text:The Molar Mass of a Volatile Liquid
Making the substitution for n in the ideal gas law, equation 1 becomes:
m
(Equation 3)
M
Rearranging equation 3, the molar mass, M, can be calculated:
PV
gas, a
M =
Show your calculations below:
=
mRT
PV
RT
(Equation 4)
20 L, at standard temperature and presure (STP)
drogen at STP?
28.00 L. What
4
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