Discussion:
1. Various indicators of a chemical reaction were observed during this experiment. The color of the compound changed, and a new substance was formed, magnesium oxide. As an alteration in chemical bonding and composition has occurred, it can be concluded that this was in fact a chemical reaction
2. As the law of conservation of mass indicated, matter cannot be created nor destroyed, but can change form. Therefore the mass of the magnesium prior to the reaction must be equal to the mass of magnesium within the compound, Mg(II)O. Based on this principle, it is possible to calculate the mass of oxygen that reacted with the magnesium:
G: mass of Mg(II)O = 0.20 g mass of magnesium = 0.13 g
R: Mass of oxygen:?
A: Mass of magnesium oxide …show more content…
Percentage composition of O within Mg(II)O = ?
A: Percentage composition of Mg within Mg(II)O = mass of Mg/mass of Mg(II)O Percentage composition of O within Mg(II)O = mass of O/mass of Mg(II)O
S: Percentage composition of Mg within Mg(II)O = 0.13 g ÷ 0.20 g = 65.0 % Percentage composition of O within Mg(II)O = 0.07 g ÷ 0.20 g = 35.0 %
P: The percentage composition of Mg within Mg(II)O is equivalent to 65.0% and the percentage composition of O within Mg(II)O is equivalent to 35.0% if values are used from observations of the experiment
4. As the observation results have revealed, despite a minor margin of error of approximately 4.70 %, the law of definite proportions is confirmed through the analysis of this chemical reaction (synthesis) as the percentage composition of mass of magnesium oxide derived from the periodic table data, and the conducted experiment are extremely close. This minuscule difference will later be explained in the sources of …show more content…
After analyzing atmospheric gasses, “air” is comprised of 78.09% nitrogen, 20.95% oxygen, 0.93% argon, 0.039% carbon dioxide, and small amounts of other gases. Therefore, the only likely gas that can react with the magnesium is nitrogen. The compound that can be formed as a result is Mg(II)3N2. Theoretically; magnesium would have a higher percentage composition which is approximately 72.24%. However, in the process of this experiment, pure H2O in the form of distilled water was used to wash excess Mg(II)O back into the crucible. If Mg(II)3N2 was to form, the water would react with it and form magnesium hydroxide and ammonia. The reheating was then done in order to release water from the magnesium hydroxide hence the extremely slight vapor released. After the water is released, the magnesium hydroxide is decomposed to water vapor and magnesium oxide and the ammonia gas is released as well. Conclusively, the mass composition would not alter because even when he magnesium reacts with nitrogen, the experiment process causes it to turn into the Mg(II)O
1. Various indicators of a chemical reaction were observed during this experiment. The color of the compound changed, and a new substance was formed, magnesium oxide. As an alteration in chemical bonding and composition has occurred, it can be concluded that this was in fact a chemical reaction
2. As the law of conservation of mass indicated, matter cannot be created nor destroyed, but can change form. Therefore the mass of the magnesium prior to the reaction must be equal to the mass of magnesium within the compound, Mg(II)O. Based on this principle, it is possible to calculate the mass of oxygen that reacted with the magnesium:
G: mass of Mg(II)O = 0.20 g mass of magnesium = 0.13 g
R: Mass of oxygen:?
A: Mass of magnesium oxide …show more content…
Percentage composition of O within Mg(II)O = ?
A: Percentage composition of Mg within Mg(II)O = mass of Mg/mass of Mg(II)O Percentage composition of O within Mg(II)O = mass of O/mass of Mg(II)O
S: Percentage composition of Mg within Mg(II)O = 0.13 g ÷ 0.20 g = 65.0 % Percentage composition of O within Mg(II)O = 0.07 g ÷ 0.20 g = 35.0 %
P: The percentage composition of Mg within Mg(II)O is equivalent to 65.0% and the percentage composition of O within Mg(II)O is equivalent to 35.0% if values are used from observations of the experiment
4. As the observation results have revealed, despite a minor margin of error of approximately 4.70 %, the law of definite proportions is confirmed through the analysis of this chemical reaction (synthesis) as the percentage composition of mass of magnesium oxide derived from the periodic table data, and the conducted experiment are extremely close. This minuscule difference will later be explained in the sources of …show more content…
After analyzing atmospheric gasses, “air” is comprised of 78.09% nitrogen, 20.95% oxygen, 0.93% argon, 0.039% carbon dioxide, and small amounts of other gases. Therefore, the only likely gas that can react with the magnesium is nitrogen. The compound that can be formed as a result is Mg(II)3N2. Theoretically; magnesium would have a higher percentage composition which is approximately 72.24%. However, in the process of this experiment, pure H2O in the form of distilled water was used to wash excess Mg(II)O back into the crucible. If Mg(II)3N2 was to form, the water would react with it and form magnesium hydroxide and ammonia. The reheating was then done in order to release water from the magnesium hydroxide hence the extremely slight vapor released. After the water is released, the magnesium hydroxide is decomposed to water vapor and magnesium oxide and the ammonia gas is released as well. Conclusively, the mass composition would not alter because even when he magnesium reacts with nitrogen, the experiment process causes it to turn into the Mg(II)O