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# How can I calculate the empirical formula of magnesium oxide?

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Electromagnetic Frequencies and Quantum Energy Analysis not available. Effects of Temperature and Concentration on reaction rates. Click to download the lab handout. Follow the presentations directions to be successful. Follow the directions on the hand out to be successful Put the data tables into your SiLL. Cu Again spg Discovering Bond Properties make up. Magnesium oxide make up lab. Make Up Cu Again Lab spg For the data listed above, calculate the mass of the product, then click here to check your answer.

Since the product of your reaction should be pure magnesium oxide containing magnesium and oxygen , and the initial material taken was pure elemental magnesium , the mass of oxygen reacted should just be the difference in these two masses. Using the data above, calculate the mass of oxygen reacted with the sample of magnesium taken, and then click here to check your answer.

The number of moles of magnesium reacted is based on the mass of magnesium taken and the molar mass of magnesium For the data above, calculate the number of moles of magnesium reacted, then click here to check your answer. The number of moles of oxygen atoms contained in 0. Note that oxygen atoms are found in MgO individually…. Calculate the number of moles of oxygen atoms contained in 0.

The empirical formula represents the smallest whole number ratio of the types of atoms in a compound. On an experimental bases, we have found that 0. This means that the number of oxygen atoms that have combined per magnesium atom is given by the ratio.

Using tongs, transfer the crucible and its cover to the clay triangle. See if you can identify the materials list above in the picture. Begin heating them with the Bunsen burner. Adjust the burner to obtain a blue flame having an inner lighter blue cone. The tip of the cone is the hottest part of the flame; use this part of the flame to heat the crucible red hot.

After heating the crucible, cool it in place on the ringstand for about five minutes to room temperature. Using the digital balance, weigh the crucible and cover to the nearest milligram. Place the magnesium sample into the crucible and then weigh the crucible, cover and sample. Record this mass and the physical appearance of the magnesium metal in your notebook.

Notice that you can't merely tare the crucible and cover. Cover the crucible with its lid and place it inside the clay triangle supported by a ring and ringstand see demo model. If the metal is burning, do not look directly at it, but replace the lid and continue heating gently until flames are no longer visible. Remove the lid and heat the crucible with the hottest part of the flame for 5 minutes. Record the physical appearance of the residue.

When the crucible and its contents have cooled after five minutes , weigh them to the nearest milligram and record this mass in your notebook. Use the same digital balance you used for the previous massing. Dispose of the magnesium product in the container designated for waste disposal.

Clean the crucible and cover. And now for the hints on how to set up your lab book: Determination of the empirical formula of the product of magnesium heating. Please write a sentence or two stating the goal of this experiment, based on the information above.

## Main Topics

The empirical formula of a compound gives the lowest whole-number ratio of the constituent atoms that is consistent with the mass ratios measured by experiment. In this lab, magnesium metal (an element) is oxidized .

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empirical formula. Example: Suppose that we want to determine the empirical formula of the oxide that formed when we ignited g of aluminum (Al) in an open container to produce a compound of Al and O that weighed g. The gain in mass is due to the presence of oxygen atoms that combined with the aluminum atoms in the reaction.