Hi guys, so we recently did a lab where we put a strip of Magnesium Carbonate in a crucible with a lid on, weighed it and then put it over a bunsen burner for a while to let it oxidise. After that, we weighed it again. Here are my results: Crucible + Lid =34.07g
Crucible + Lid + Magnesium = 34.2g
Crucible + Lid + Contents after reaction = 34.21g.
I am now required to write up a lab report with Aim, summarise the reaction in equation, Tabulate raw results and process your results showing clearly structures calculations. For the calculations I am required to know the weight of the Mg and the Oxygen after the reaction to work out the Empirical Formula. My question is, would the weight of the oxygen be 0.01g? Please help. Thanks (I need an answer by the 14th of jan)
To calculate the weight of oxygen in the reaction, we need to use the law of conservation of mass. According to this law, the mass of the reactants should be equal to the mass of the products in a chemical reaction.
Let's start by calculating the weight of magnesium. Weighing the crucible, lid, and magnesium together before the reaction gives a mass of 34.2g. The mass of the empty crucible and lid is 34.07g.
So, the mass of magnesium can be calculated by subtracting the initial mass (34.07g) from the mass after adding magnesium (34.2g).
Mass of magnesium = 34.2g - 34.07g
= 0.13g
Now, let's calculate the weight of the oxygen. Weighing the crucible, lid, and contents after the reaction gives a mass of 34.21g.
To find the weight of oxygen, we need to subtract the combined weight of the crucible, lid, and magnesium from the weight after the reaction.
Weight of oxygen = Mass after reaction - (Mass of crucible + Mass of magnesium)
Weight of oxygen = 34.21g - (34.07g + 0.13g)
= 34.21g - 34.20g
= 0.01g
Therefore, you are correct. The weight of oxygen in the reaction is indeed 0.01g.
Now, for the empirical formula calculations, you will need the molar masses of magnesium and oxygen. The molar mass of magnesium (Mg) is approximately 24.31 g/mol, and the molar mass of oxygen (O) is approximately 16.00 g/mol.
To find the empirical formula, you will need to convert the weights of magnesium and oxygen to moles using their respective molar masses. Then, divide the moles of each element by the smallest number of moles calculated to obtain the simplest whole-number ratio of atoms.
I hope this helps you with your lab report! If you have any more questions, feel free to ask.