Abstract In this lab, to help better understand the concepts of gram atomic masses and empirical formulas, we found the gram atomic masses and empirical formula of a binary compound.
The two compounds should form a definite whole number ratio by mass. This ratio will also help determine the subscripts of the elements in the empirical formula. Errors in this experiment can stem from measuring wrong or doing equations incorrectly.Procedure First thing to do is to gather the equipment and materials needed for this lab.
These include a magnesium ribbon, a crucible and cover, ring stand, iron ring, crucible tongs, burner, balance, and safety goggles. Once all the items are ready and available, then the lab can begin. Measure the mass of the crucible by itself and record the data. Then take the piece of magnesium ribbon and break it into small bits.
Place the bits into the crucible and measure them together. Then place the lid on the top and heat it with the bits inside for 2 minutes. Then use the tongs to tilt the cover and provide an opening. Then heat it up again for 10 minutes. Once enough time has passed, turn off the burner and allow the crucible to cool. Then measure it again.
Once everything is cool enough to touch, put away all the materials and examine the data.Results Utilizing the observations and data acquired, completing the calculations and finding the empirical formula was easily accomplished. With the data acquired from the calculations, it was easy to find the the ratio of g-atoms of Mg to g-atoms of O: DataMass of empty crucible - 36.2 gramsMass of crucible (with Mg) - 36.5 gramsMass of crucible (with O) - 37.3 gramsCalculationsMass of Magnesium used - 3 gramsMass of reacted Oxygen - 8 gramsNumber of g-atoms of Mg used - 0125Number of g-atoms of O reacted - 05Ratio of g-atoms of Mg to g-atoms of O – 1:4This means that for every one atom of Magnesium, there are four atoms of Oxygen.
This would make the empirical formula of this compound MgO4.
