Magnesium oxide conclusion

The MgO has completely dissolved in the HCl. Therefore, the average temperature high for the MgO and HCl solution in trial 2 was Place the strip of magnesium in a crucible and weigh it.

A lot of gas is forming. Therefore, the average temperature high for the Mg and HCl solution in trial 2 was If we burn 0.

Set up the cricible on a tripod above a Bunsen burner and begin heating. However, this would explain the small error in this experiment as the discrepancies were not that high.

Through experimentation it was found that the enthalpy of change for the combustion of magnesium is HCl is clear and has a slight odour. Prepare a strip of magnesium about 10 cm long.

MgO is small, white granular pieces, a fine white powder. Place the crucible containing the magnesium in the pipe clay triangle and put the lid on. The Mg has completely dissolved in the HCl. There were two holes on the lid of the calorimeter and one was being used for the thermometer, however the second, although very small, was left open.

The increase in mass is due to the fact that oxygen from the air has combined with the magnesium to make magnesium oxide, MgO. It is evident that the two equations which were used in this experiment were exothermic since the enthalpy of change that resulted was a negative value, therefore the experiment was successful.

In the future the procedure should emphasize the importance of measuring and pouring the magnesium after the HCl has been measured and poured into the calorimeter, this would prevent other reactions from occurring.

Many bubbles are forming. Once again, the loss of heat would have resulted in a lower enthalpy value. The electronic balance, or any balance, should be placed at Magnesium oxide conclusion work station and as soon as the right amount of magnesium has been measured out it should be poured into the calorimeter immediately.

You may see the magnesium begin to flare up. It is worth evaluating what they have done as there are several reasons why their results may be disappointing: They could also calculate the increase in mass mass 3 - mass 2which corresponds to the mass of oxygen.

Since the percent error is a very small value it is evident that the experiment was a success, however this does not mean that it was perfect. Repeat this step until the mass readings are consistent. Having done this for both elements, they should find the ratio between the two by dividing them both by the smallest number.

If the lid is off for too long then the magnesium oxide product will begin to escape. Using stoichiometry, we can convert this eqation into an equation with moles: Both of these conditions would have lead to a lower final temperature value.

In the future, to prevent this, the partner that is not pouring the magnesium should hold the lid close to the calorimeter and only open it at a small angle so that there is just enough space for the other partner to pour in the magnesium or magnesium oxide.

Replace the lid if it appears that you are losing some product.The change in mass when magnesium burns. Finding the formula of magnesium oxide. METHOD 1 To find the formula of magnesium oxide, students will need the mass of the magnesium and the mass of the oxygen.

They will also require the relative atomic masses.

Heat of Reaction for the Formation of Magnesium Oxide Lab Answers

Magnesium is 24 and oxygen is A strip of magnesium metal reacts with oxygen in the air to produce magnesium oxide. In order to experimentally determine the percentage composition and empirical formula of magnesium oxide, a piece of magnesium is heated strongly to react with the oxygen in the air.

Conclusion: Read through the introduction and purpose of this lab. Write a 3 sentence summary that highlights what was accomplished during this activity and any errors that were made.

It should be clear you understand why you did the lab. Class Set: Do not write on. Essays - largest database of quality sample essays and research papers on Magnesium Oxide Conclusion. Determining the Empirical Formula of Magnesium Oxide Experiment. Weight of oxygen gained % of magnesium in the oxide % of oxygen in the oxide Mean % magnesium: Results/ Conclusion:2/5(4).

Lab 2 - Determination of the Empirical Formula of Magnesium Oxide Goal and Overview The quantitative stoichiometric relationships governing mass and amount will be studied using the combustion reaction of magnesium metal.

Magnesium oxide conclusion
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