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To reach molar ratios, the number of moles of magnesium and oxygen were reached and simplified into the lowest whole number ratios. The empirical formula of magnesium oxide was then decided. During data processing, the percentage uncertainties associated with masses were found so that the percentage uncertainties of the number of moles were concluded.
4.Number of moles of oxygen atoms that were used. = 0.0080Mole (the number of moles of oxygen = mass / atomic weight . The atomic weight of magnesium is 16.0 g / mole ) 5.Simplest ratio: Mg = 0.0096Mole = 1.2 0.0080Mole Oxygen = 0.0080mole = 1 0.0080mole Multiply by
When the temperature is -273?, the volume will be 0. However, gases do not really reach a 0 volume but the spaces between molecules approach 0. We use the unit called Kelvin (K) because absolute zero means the temperature never goes down more than -273?
o They are the salt makers. o As we go down the group, atomic, ionic and covalent radii increase. Ionisation energies for this group are the second highest in the periodic table. o As we go down the group, the reactivity of the halogen decreases, but the halide's increases.
The most diluted concentration of copper sulfate (0.2 M) shows the lowest potential difference (voltage) between the two half-cells. In contrast, the most concentrated copper sulfate solution (1.0 m) shows the highest potential difference between the two-half cells. However, potential difference remained constant (0.83 V)
According to the formula, the pressure of a book had 251g/cm� (1440/5.73 = 251g/cm�). Therefore, the pressure will be constantly changed by the number of books. It is not the end of the pressure. I had to add the total pressure on the piston equals the pressure from the books plus the atmospheric pressure.
RAW DATA PROCESSING: For Part X, Trial 1 To obtain an estimation of the maximum temperature reached in the trial, a graph is drawn which shows all the progressing and regressing values of temperature against time. Following that, a best fit line is drawn for all the progressing and then the regressing values of temperature.
Calculate the percentage composition of magnesium oxide using your experimental data from Part A. The percentage composition of magnesium is 61.76% and the percentage composition of oxygen is 38.24%. 1. Calculate the percentage composition of magnesium oxide using your experimental data from Part B.
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