Thomas HayesInvestigating the rate of reactionsAim: To
investigate the effect of increasing the concentration of HCl has
on the rate of reaction between Mg & HCl. Mg (g) + 2HCl (l)
MgCl2 (aq) + H2 (g) Introduction: The purpose of this experiment is
to investigate the effect of increasing the concentration of HCl
has on the rate of reaction between Mg and HCl. In order to do
this, I will dilute 1 molar HCl to 5 different concentrations (.2
M, .4 M, .6 M, .8 M and 1 M) and measure their rate of reaction
with Mg. Hypothesis: We can expect the rate of reaction to increase
as the concentration of HCl increases. Variables:Independent
variable: Concentration of HClDependent variable: The change in gas
pressure of the reaction mixtureControlled: Amount of HCl used in
each experiment A burette was used to make sure only 20 mL of HCl
was put into the flask. Temperature of HCl All of the HCl was room
temperature, if they had different temperatures the results would
be altered due to temperature changing the rate of the reaction.
Amount of Mg used in each experiment An electric scale was used to
measure 1.00 g of Mg for each trial. Temperature The temperature
was room temperature and the air conditioner was off while all
windows were closed. Experimenter I will be conducting all of the
experiments. Experimenter changes could cause error and alter the
results. Apparatus: 1M HCl- Magnesium Strips .8M HCl .6M HCl .4M
HCl .2M HCl Electric scale 300 mL beaker Burette Graduated Cylinder
Vernier (along with Gas Pressure Sensor) Flask Funnel Burette stand
Glass plateUncertainties: Electric scale = 0.01 Graduate cylinder =
0.1 Burette = 0.1 Magnesium strips = 0.01Method: 1. Gather the
burette, flask, funnel, glass plate, Vernier with gas pressure
sensor and burette stand. 2. Pour 50 mL of desired HCl into the
burrette while its in the burette stand. 3. Weigh 1.00 g of Mg on
the electric scale. If you use a glass plate to put the Mg on while
you measure it be sure to zero out the scale.4. Put 20 mL of HCl
into the flask. 5. Prepare the Mg to be put into the flask and be
sure to quickly put the gas pressure sensor on the flask as soon as
the Mg is put into the flask. So you can avoid losing data and
error. Also, make sure the gas pressure sensor is closed and not
open.6. Put the 1.00 gram of Mg into the flask with 20 mL of HCl.
Then quickly but the gas pressure sensor onto the flask. 7. Let the
reaction run for 105 seconds then open the gas pressure sensor.8.
Remove the gas pressure sensor and repeat the steps for each trial.
Results:*NOTE* The amount of time each trial ran was inconsistent
which could contribute to a lot of the error. Due to the
inconsistent times I recorded the pressure at 20, 40, 60, 80 and
100 seconds of each reaction.
Raw Data:0.2 M HCl Trial 1Analysis: 0 seconds 99.22 kPa 20
seconds 104.32 kPa40 seconds 107.73 kPa60 seconds 110.18 kPa80
seconds 112.05 kPa100 seconds 113.47 kPa
0.2 M HCl Trial 2
Analysis:0 seconds 99.35 kPa 20 seconds 103.54 kPa40 seconds
107. 08 kPa60 seconds 109.66 kPa80 seconds 111.86 kPa100 seconds
113.47 kPa
0.2 M Trial 3
Analysis:0 seconds 99.47 kPa20 seconds 105.80 kPa40 seconds
109.80 kPa60 seconds 111.66 kPa80 seconds 113.60 kPa100 seconds
115.34 kPa
0.4 M HCl Trial 1
Analysis:0 seconds 99.02 kPa20 seconds 112.12 kPa40 seconds
120.63 kPa60 seconds 125.79 kPa80 seconds 129.27 kPa100 seconds
131.79 kPa
0.4 M HCl Trial 2
Analysis:0 seconds 99.02 kPa20 seconds 109.93 kPa40 seconds
117.86 kPa60 seconds 123.21 kPa80 seconds 127.02 kPa100 seconds
129.53 kPa
0.4 M HCl Trial 3
Analysis:0 seconds 99.28 kPa20 seconds 110.12 kPa40 seconds
118.56 kPa60 seconds 123.86 kPa80 seconds 127.08 kPa100 seconds
129.40 kPa
0.6 M HCl Trial 1
Analysis: 0 seconds 99.35 kPa20 seconds 119.14 kPa40 seconds
129.79 kPa60 seconds 136.24 kPa80 seconds 140.88 kPa100 seconds
144.56 kPa
0.6 M HCl Trial 2
Analysis:0 seconds 99.47 kPa20 seconds 118.18 kPa40 seconds
128.37 kPa60 seconds 134.43 kPa80 seconds 138.30 kPa100 seconds
141.33 kPa
0.6 M HCl Trial 3
Analysis:0 seconds 99.35 kPa20 seconds 117.15 kPa40 seconds
127.60 kPa60 seconds 133.66 kPa80 seconds 138.04 kPa100 seconds
140.69 kPa
0.8 M HCl Trial 1
Analysis:0 seconds 99.47 kPa20 seconds 139.46 kPa40 seconds
154.88 kPa60 seconds 163.39 kPa80 seconds 169.19 kPa100 seconds
172.93 kPa
0.8 M HCl Trial 2
Analysis:0 seconds 99.54 kPa20 seconds 141.46 kPa40 seconds
156.17 kPa60 seconds 164.36 kPa80 seconds 169.19 kPa100 seconds
172.68 kPa
0.8 M HCl Trial 3
Analysis:0 seconds 99.28 kPa20 seconds 135.98 kPa40 seconds
152.10 kPa60 seconds 159.65 kPa80 seconds 164.94 kPa100 seconds
168.68 kPa
1.0 M HCl Trial 1
Analysis: 0 seconds 99.02 kPa20 seconds 150.75 kPa40 seconds
171.13 kPa60 seconds 181.58 kPa80 seconds 187.64 kPa100 seconds
189.83 kPa
1.0 M HCl Trial 2
Analysis:0 seconds 99.47 kPa20 seconds 152.88 kPa40 seconds
172.87 kPa60 seconds 183.00 kPa80 seconds 188.93 kPa100 seconds
192.15 kPa
1.0 M HCl Trial 3
Analysis: There was a little error in the beginning of the
reaction because the gas sensor pressure allowed a little of the
gas out from the reaction. 0 seconds 99.09 kPa20 seconds 139.53
kPa40 seconds 159.71 kPa60 seconds 168.48 kPa80 seconds 173.26
kPa100 seconds 176.16 kPa
Processed Data:
