Equation 2Mg+O2= 2MgO
Lab data:
Magnesium ribbon= .04 grams
Magnesium Oxide= .09
2. Using the initial mass of magnesium, calculate the moles of oxygen and then moles of magnesium oxide produced. What is the mole ratio of the reactants?
3. Calculate the mass of magnesium oxide from the initial mass of magnesium.
4. Calculate the percent error, using the calculated mass of magnesium oxide and the actual mass of magnesium oxide produced in the experiment.
What are you suppose to calculate?
To answer these questions, we need to follow the steps given in the question and use the given data.
2. To calculate the moles of oxygen, we need to use the mole ratio of the reactants. From the balanced equation 2Mg + O2 = 2MgO, we can see that the mole ratio of Mg to O2 is 2:1. So, for every 2 moles of magnesium (Mg), there will be 1 mole of oxygen (O2) consumed.
Given the initial mass of magnesium ribbon as 0.04 grams, we can calculate the moles of magnesium using its molar mass. The molar mass of magnesium (Mg) is 24.31 grams/mol.
Moles of magnesium (Mg) = (Mass of magnesium / Molar mass of magnesium)
= (0.04 g / 24.31 g/mol)
≈ 0.0016 moles of magnesium
Since the mole ratio of Mg to O2 is 2:1, the moles of oxygen (O2) can be calculated as:
Moles of oxygen (O2) = 0.0016 moles of magnesium / 2
= 0.0008 moles of oxygen
Next, we can calculate the moles of magnesium oxide produced.
From the balanced equation, we can see that 2 moles of magnesium oxide (MgO) are produced for every 2 moles of magnesium (Mg) consumed.
Moles of magnesium oxide (MgO) = Moles of magnesium (Mg)
= 0.0016 moles of magnesium
So, the moles of magnesium oxide (MgO) produced is 0.0016 moles.
The mole ratio of the reactants, Mg to O2, is 2:1.
3. Now, we can calculate the mass of magnesium oxide (MgO) produced from the initial mass of magnesium.
From the balanced equation, we know that 2 moles of magnesium oxide (MgO) are produced for every 2 moles of magnesium (Mg) consumed.
Mass of magnesium oxide (MgO) = Moles of magnesium oxide (MgO) * Molar mass of magnesium oxide (MgO)
The molar mass of magnesium oxide (MgO) is 40.31 g/mol.
Mass of magnesium oxide (MgO) = 0.0016 moles of magnesium oxide * 40.31 g/mol
≈ 0.0645 grams of magnesium oxide
So, the mass of magnesium oxide produced from the initial mass of magnesium is approximately 0.0645 grams.
4. Finally, we can calculate the percent error using the calculated mass of magnesium oxide and the actual mass of magnesium oxide produced in the experiment.
Given actual mass of magnesium oxide produced in the experiment as 0.09 grams.
Percent error = [(Actual mass - Calculated mass) / Actual mass] * 100
= [(0.09 g - 0.0645 g) / 0.09 g] * 100
= [0.0255 g / 0.09 g] * 100
≈ 28.33%
So, the percent error is approximately 28.33%.