Magnesium Volume Lab
The volume of one mole of gas under conditions of room temperature and pressure
Data collection and processing
Quantitative data in table with units and uncertainties | Mass of Magnesium(Mg) (g) | Volume of Hydrogen (H₂) (cm³) | 1st trial | 0.040 | 39.9 | 2nd trial | 0.040 | 40.3 | 3rd trial | 0.035 | 36.5 |
Quantitative data:
The Magnesium was silvery-white, lustrous and relatively flexible before being placed in the burette. Whilst reacting with the hydrochloric acid, it dissolved and bubbles were visible. The hydrochloric acid slowly diffused downwards.
Calculations:
Volume of un-diffused hydrochloric acid = 25 cm³
Average mass of magnesium = 0.038 g
Average volume of diffused hydrochloric acid = 11.1 cm³
Average volume of …show more content…
The average volume of hydrogen produced was found to be 38.9 cm³. This was calculated by finding the difference of the un-diffused hydrochloric acid plus water from the diffused hydrochloric acid (50 cm³ -11.1 cm³). This result is in disagreement to the original equation and thus it is clear that a lot of errors were present during the experiment as the result did not come to 24, but rather 38.9 cm³.
Weaknesses and limitations * The magnesium strips were all not the same weight and thus this would mean either more or less reaction, meaning more or less hydrogen gas produced. * The balances had a systematic error of ± 0.05 g and thus this will have introduced errors in the mass measurements. * Loss of some of the hydrochloric acid due to spillage, or some may have been left off in the measuring cylinder. * Since magnesium was the limiting reagent, it is uncertain of whether or not it had all reacted in the experiment. Bubbles also made it difficult to get the most accurate
Data collection and processing
Quantitative data in table with units and uncertainties | Mass of Magnesium(Mg) (g) | Volume of Hydrogen (H₂) (cm³) | 1st trial | 0.040 | 39.9 | 2nd trial | 0.040 | 40.3 | 3rd trial | 0.035 | 36.5 |
Quantitative data:
The Magnesium was silvery-white, lustrous and relatively flexible before being placed in the burette. Whilst reacting with the hydrochloric acid, it dissolved and bubbles were visible. The hydrochloric acid slowly diffused downwards.
Calculations:
Volume of un-diffused hydrochloric acid = 25 cm³
Average mass of magnesium = 0.038 g
Average volume of diffused hydrochloric acid = 11.1 cm³
Average volume of …show more content…
The average volume of hydrogen produced was found to be 38.9 cm³. This was calculated by finding the difference of the un-diffused hydrochloric acid plus water from the diffused hydrochloric acid (50 cm³ -11.1 cm³). This result is in disagreement to the original equation and thus it is clear that a lot of errors were present during the experiment as the result did not come to 24, but rather 38.9 cm³.
Weaknesses and limitations * The magnesium strips were all not the same weight and thus this would mean either more or less reaction, meaning more or less hydrogen gas produced. * The balances had a systematic error of ± 0.05 g and thus this will have introduced errors in the mass measurements. * Loss of some of the hydrochloric acid due to spillage, or some may have been left off in the measuring cylinder. * Since magnesium was the limiting reagent, it is uncertain of whether or not it had all reacted in the experiment. Bubbles also made it difficult to get the most accurate