This preview shows pages 1–3. Sign up to view the full content.
Experiment 5 The Molar Volume of Gases
Pre Lab Questions
1.
Molar volume= molar mass/density= 17.034 (g/mol)/0.76(g/L)=22 mol/L.
Therefore
the units of molar volume are mol/L.
2. Molar volume= 31.999 (g/mol)/1.429 (g/L)=22.392 mol/L
3. 48.1 g CH4/16 (g/mol)= 3.01 mol
V=(3.01)(.0821)(27)= 67.5 L
4. A) To determine mass and number of moles, find the molar mass and convert to moles.
B) To determine the volume of oxygen produced, we can calculate the volume of O2 in
L/mol.
5.
P total is determined by adding P O2 and P H20 together.
You must equalize the
pressure inside and outside the flask to determine the total because it keeps the water
level the same.
6.
X18.65 torr/ 19.827 torr18.65= 21.6 degrees21 degrees/22 degrees21 degrees=
19.36 torr
7. 22.3 degrees C22 degrees C/ 23 degrees C22 degrees C= x19.827 torr/21.068 torr
19.827 torr= 20.199 torr
8.
A) Determine the number of moles by looking at the equation and finding molar mass.
B) To find the volume of hydrogen, take the molar mass and divide by density.
Find
The volume of H2 produced at known temperatures.
9.
V2= V1(P1/P2)(T2/T1)
V2=110 mL(750 torr/760 torr)(273 K/293 K)
(108.55)(.93174)= V2=101 mL
Introduction
The purpose of the lab is to learn how to find the molar volume of gases.
The lab is also
how to measure the volumes of gases and calculating the molar volume of gases using the
ideal gas law and the law of partial pressures.
Data
Part 1:
1.
The first step is to clean the glassware with soap and water.
2.
Then we had to set up the experiment as shown in the diagram in the book.
We
measured 20 mL of 3% solution in a graduated cylinder and poured it into a 250 mL
Erlenmeyer flask.
Then it was measured and pour approximately 4.5 mL of 3M FeCl3 in
a test tube and it was lowered into a 250 mL Erlenmeyer flask.
This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document 3.
The next step involved filling a 500 mL Erlenmeyer flask to the neck with water and
fill the 600 mL beaker about onethird full with tap water.
Then air was forced into the
This is the end of the preview. Sign up
to
access the rest of the document.
This note was uploaded on 09/30/2008 for the course CHEM 1A/1B taught by Professor Neuman during the Fall '06 term at UCSB.
 Fall '06
 NEUMAN

Click to edit the document details