Chemistry IA
Raw Data:
Table 1.1: Raw Data Table
Temperature (°C) ±0.5
Initial Mass (grams) ±0.001
Final Mass (grams)
±0.001
Initial Volume (cm³)
±0.5
Final Volume (cm³)
±0.5
Pressure
(hPa)
±0.5
24.0
0.000
0.072
0.1
60.4
1008.0
24.0
0.000
0.060
0.1
55.9
1008.0
24.0
0.000
0.053
0.1
54.9
1008.0
24.0
0.000
0.044
0.1
45.4
1008.0
24.0
0.000
0.032
0.1
34.3
1008.0
24.0
0.000
0.025
0.1
23.3
1008.0
Table 1.2: Qualitative Data:
Before
During
After
Magnesium (Mg) strips were dull due to the oxidization. Even after sanding the strip, there were still places of oxidization.
Hydrochloric Acid (HCl) was clear, colourless and liquid.
When the Mg strip was dropped into the HCl the release of white gas could be observed due to the reaction.
The gas release caused animated fizzing.
Temperature of boiling tube increases significantly, thus we can consider the reaction as being an exothermic reaction.
Temperature gradually decreases.
The solution is clear and colourless , with no traces of the Mg strip.
Data Processing:
PV = nRT
P; Pressure - Pa
V; Volume - m3 n; Number of moles - moles
R; Gas Constant - JK-1mol-1
T; Temperature - K
Gas Constant (R) is what we are trying to calculate
Known Gas Constant: 8.31 JK-1mol-1
Sample Calculations:
Temperature needs to be converted from degree Celsius in Kelvin
Temperature in Kelvin:
°C + 273 = … K
e.g. 24.0 + 273 = 297.0 Kelvin
From the Mass we need to calculate the number of moles (n) of Magnesium (Mg)
Using the Final Mass minus the Initial Mass from the Raw Data table moles = mass/ relative atomic mass
e.g. Mols = 0.025/ 24.31 = 0.001028
Also from the formula [Mg + 2HCl MgCl2 + H2]
Number of moles of H2 is the same and Mg. Therefore, moles of H2 = 0.001028
Volume needs to be converted from cm³ to m³
(Final volume – Initial volume) * 10-6
e.g. 23.2 * 10-6 = 0.0000232 m³
Pressure needs to be converted from hPa to Pa hPa * 100
Table 1.1: Raw Data Table
Temperature (°C) ±0.5
Initial Mass (grams) ±0.001
Final Mass (grams)
±0.001
Initial Volume (cm³)
±0.5
Final Volume (cm³)
±0.5
Pressure
(hPa)
±0.5
24.0
0.000
0.072
0.1
60.4
1008.0
24.0
0.000
0.060
0.1
55.9
1008.0
24.0
0.000
0.053
0.1
54.9
1008.0
24.0
0.000
0.044
0.1
45.4
1008.0
24.0
0.000
0.032
0.1
34.3
1008.0
24.0
0.000
0.025
0.1
23.3
1008.0
Table 1.2: Qualitative Data:
Before
During
After
Magnesium (Mg) strips were dull due to the oxidization. Even after sanding the strip, there were still places of oxidization.
Hydrochloric Acid (HCl) was clear, colourless and liquid.
When the Mg strip was dropped into the HCl the release of white gas could be observed due to the reaction.
The gas release caused animated fizzing.
Temperature of boiling tube increases significantly, thus we can consider the reaction as being an exothermic reaction.
Temperature gradually decreases.
The solution is clear and colourless , with no traces of the Mg strip.
Data Processing:
PV = nRT
P; Pressure - Pa
V; Volume - m3 n; Number of moles - moles
R; Gas Constant - JK-1mol-1
T; Temperature - K
Gas Constant (R) is what we are trying to calculate
Known Gas Constant: 8.31 JK-1mol-1
Sample Calculations:
Temperature needs to be converted from degree Celsius in Kelvin
Temperature in Kelvin:
°C + 273 = … K
e.g. 24.0 + 273 = 297.0 Kelvin
From the Mass we need to calculate the number of moles (n) of Magnesium (Mg)
Using the Final Mass minus the Initial Mass from the Raw Data table moles = mass/ relative atomic mass
e.g. Mols = 0.025/ 24.31 = 0.001028
Also from the formula [Mg + 2HCl MgCl2 + H2]
Number of moles of H2 is the same and Mg. Therefore, moles of H2 = 0.001028
Volume needs to be converted from cm³ to m³
(Final volume – Initial volume) * 10-6
e.g. 23.2 * 10-6 = 0.0000232 m³
Pressure needs to be converted from hPa to Pa hPa * 100