Calculator
The Molar Volume of a Gas
5
In this experiment, you will determine the molar volume of a gas by conducting a chemical
reaction that produces a gas, as shown in the reaction equation below.
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
You will react a known mass of solid magnesium with an excess of hydrochloric acid, in a sealed
vessel, and use the pressure change to calculate molar volume at STP.
OBJECTIVES
In this experiment, you will



Measure the gas production of a chemical reaction by a pressure change.
Determine the molar volume of the gas produced in the reaction.
Calculate the molar volume of a gas at STP.
Figure 1
MATERIALS
LabPro or CBL 2 interface
TI graphing calculator
Vernier Gas Pressure Sensor
Temperature Probe
600 mL beaker
10 mL graduated cylinder
magnesium ribbon, pre-cut
Advanced Chemistry with Vernier
3.0 M hydrochloric acid, HCl, solution
small beaker for HCl solution
analytical balance
125 mL Erlenmeyer flask
20 mL gas syringe
plastic tubing with two Luer-lock connectors
rubber stopper assembly with two-way valve
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Calculator 5
PRE-LAB EXERCISE (do at end of lab!)
Obtain the 125 mL Erlenmeyer flask that you will use for the experiment. Determine and record
the available volume of the flask that the hydrogen gas will occupy as it is produced from the
reaction of the solid magnesium and the hydrochloric acid solution. Account for the following
items when you determine the volume of your flask:


A 125 mL flask does not have a volume of precisely 125 mL.
During the experiment, you will seal the flask with a rubber stopper and the stopper will
occupy some of the volume of the flask.
 You will add 5 mL of solution (3.0 M HCl solution) to the flask.
PROCEDURE
1. Obtain and wear goggles.
2. Obtain a piece of magnesium ribbon. Find its mass using the analytical balance. Place the
piece of magnesium ribbon in a clean and dry 125 mL Erlenmeyer flask.
3. Prepare a room temperature water bath in a 600-mL beaker. The bath should be deep enough
to completely cover the gas level in the Erlenmeyer flask.
4. Connect a Gas Pressure Sensor to Channel 1 of the LabPro or CBL 2 interface. Connect a
Temperature Probe to Channel 2 of the interface. Use the link cable to connect the interface
to the TI graphing calculator.
5. Use the clear tubing to connect the white rubber stopper to the Gas Pressure Sensor. (About
one-half turn of the fittings will secure the tubing tightly.) Twist the white stopper snugly
into the neck of the Erlenmeyer flask to avoid losing any of the hydrogen gas that will be
produced in the reaction (see Figure 1). Important: Close the valve on the white stopper by
turning the white handle so it is perpendicular with the valve stem.
6. Obtain a small amount of 3.0 M hydrochloric acid. CAUTION: Handle the hydrochloric
acid with care. It can cause painful burns if it comes in contact with the skin. Draw 5 mL of
HCl solution into the 20 mL syringe. Thread the syringe onto the two-way valve on the white
stopper (see Figure 1). Submerge the Erlenmeyer flask into the water bath. Position the
Temperature Probe in the water bath so that the tip of the probe is not touching the beaker.
7. Set up the calculator and interface for the Gas Pressure Sensor and the Temperature Probe.
a. Turn on the calculator and start the DATAMATE program. Press CLEAR to reset the program.
b. Select SETUP from the Main screen. If CH 1 displays GAS PRESSURE(KPA) and CH 2
displays STAINLESS TEMP(C) proceed directly to Step 8. If it does not, continue with this
step to set up your sensors manually.
c. Press ENTER to select CH 1.
d. Select PRESSURE, and then select the proper sensor from the SELECT SENSOR menu. Select
an appropriate unit of pressure for your experiment.
e. At the Setup screen, press
once, then press ENTER . Select TEMPERATURE and select
the type of temperature probe that you are using.
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Advanced Chemistry with Vernier
The Molar Volume of a Gas
8. Set up the data collection mode.
a. To select MODE, press
or
until the cursor is to the left of MODE and press
ENTER .
b. Select TIME GRAPH from the SELECT MODE menu.
c. Select CHANGE TIME SETTINGS. Type “2”, for the time between samples in seconds, and
press ENTER .Type “150”, for the number of samples, and press ENTER .
d. Select OK twice to return to the Main screen.
9. With the flask still submerged in the water bath, select START to begin data collection. After
about 20 seconds, open the two-way valve directly below the syringe, press the plunger to
add all of the 5 mL of HCl solution to the flask, and close the two-way valve.
10. Gently swirl the flask, while keeping it immersed in the water bath, as the reaction proceeds.
Data collection will stop after 5 minutes. During the experiment, only the pressure readings
will be plotted on the graph. You may press STO to end data collection before 5 minutes
have elapsed, if the pressure readings are no longer changing.
11. Carefully remove the white stopper from the flask to relieve the pressure in the flask.
Important: Do not open the two-way valve to release the pressure in the flask.
12. Analyze the data. Temperature and pressure will be plotted on separate graphs.
a. Press ENTER to see the graph of pressure vs. time. Examine the graph and determine the
maximum pressure change. Record the pressure change, ∆P, in your data table, and then
press ENTER .
b. Press
, and then press ENTER to see the graph of temperature vs. time. Review this
graph to determine the temperature of the water bath (considered to be the temperature of
the reaction) and record this value in your data table.
c. Press ENTER , and then select MAIN SCREEN.
13. Use your text, or another appropriate reference, to find and record the water vapor pressure
for the temperature of the water bath.
14. For clean-up, neutralize any excess or spilled acid. Rinse the flask and syringe repeatedly
inside and out with water.
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Calculator 5
DATA TABLE
Mass of Mg (g)
Volume of flask (mL)
Maximum pressure (kPa)
Initial pressure (kPa)
Pressure change, ∆P (kPa)
Temperature (K)
Vapor pressure of water (kPa)
DATA ANALYSIS
1. Calculate the number of moles of magnesium that you used.
2. Use your results to calculate the molar amount of hydrogen gas that was produced in your
reaction.
3. Calculate the volume of one mole of hydrogen gas (molar volume), using your results.
Convert this value to STP.
4. Compare your calculated molar volume, at STP, with the accepted molar volume of an ideal
gas at STP, 22.4 L/mol, by calculating a percent error. If the values do not compare well,
suggest possible sources of experimental error.
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Advanced Chemistry with Vernier