Magnesium Oxide Lab
The Law of Definite Proportions states that a chemical compound contains the same element in exactly the same proportions by mass regardless of the size of the sample or source of the compound. This relates to the magnesium oxide lab because we tested out this theory to see if it is true that the law of definite proportions says that a chemical compound contains the same element in exactly the same proportions by mass regardless of the size of the sample or source of the compound. In this experiment, you first find the mass of the crucible and cover. Next, you will find the mass of crucible, cover and Mg. After that, you will crumple up the Mg and put it into the crucible and put the cover on over the bunsen burner with heating it for four min. Then you will remove the lid slightly and let it heat for another
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4 mins. Once those 4 mins are up, then you will let the container cool down until you can touch it so you can wait to find the mass of crucible, cover, and the product.
Our qualitative data of magnesium before the product is that it is a shiny, silver strip with a smooth texture and after the product the Mg was a whitish gray like powder.
Then our quantitative data for the mass of crucible and cover is 32.24g. The mass of the crucible, cover, and Mg is 32.54g and the mass of crucible cover and the product is 34.86g. Once my group found out all of those measurements, we could find the mass of the magnesium that reacted. That equation is the mass of the Mg, crucible and cover - mass of crucible and cover and that would be 32.54 - 32.24= 0.30g. After that, we found the mass of the magnesium oxide that was produced. The equation for the mass of magnesium oxide that was produced is a mass of product, crucible and cover - a mass of crucible and cover = mass of product. 34.86- 32.24= 2.64 After that we found the mass of oxygen reacted. The equation is a mass of product - mass of Mg = oxygen reacted. 2.62-0.30=1.23g of oxygen. next we found the ratio of the mass of magnesium to the mass of oxygen it would be a Mass of Mg/Mass of oxygen= a decimal 2.62/2.32=1.23g And that would lead us to find the % error. and our % error is
19%.
My data does not support the law of definite proportions because our data are far away from the best fit line which has a slope of y= 0.51*x-0.012. But our class data works because the r2=0.594 tells us that class data is almost as one with is really close to the best-fit line. Some points that could be ignored are the negative point because you can't have a negative mass. In this lab, we had 19% of error. Some of the things that could have affected the results was our piece of Mg wouldn't start. Instead of leaving it in the container we put it into the bunsen burner flame to get it started once it started we put it back into the container. The error was that some of the mass could have escaped during that time. Another thing that could lead to our error was once we got the Mg to go and it was almost cool we took it off of the stand and dropped on the counter. The error was that our mass was not quite right because we might drop some of the Mg masses before we weighted it. The third possible source of error is our mass and measurements. Because we dropped the crucible we could have lots some of our products which would affect the mass. To conclude, some of the errors that could have affected our results.
4 mins. Once those 4 mins are up, then you will let the container cool down until you can touch it so you can wait to find the mass of crucible, cover, and the product.
Our qualitative data of magnesium before the product is that it is a shiny, silver strip with a smooth texture and after the product the Mg was a whitish gray like powder.
Then our quantitative data for the mass of crucible and cover is 32.24g. The mass of the crucible, cover, and Mg is 32.54g and the mass of crucible cover and the product is 34.86g. Once my group found out all of those measurements, we could find the mass of the magnesium that reacted. That equation is the mass of the Mg, crucible and cover - mass of crucible and cover and that would be 32.54 - 32.24= 0.30g. After that, we found the mass of the magnesium oxide that was produced. The equation for the mass of magnesium oxide that was produced is a mass of product, crucible and cover - a mass of crucible and cover = mass of product. 34.86- 32.24= 2.64 After that we found the mass of oxygen reacted. The equation is a mass of product - mass of Mg = oxygen reacted. 2.62-0.30=1.23g of oxygen. next we found the ratio of the mass of magnesium to the mass of oxygen it would be a Mass of Mg/Mass of oxygen= a decimal 2.62/2.32=1.23g And that would lead us to find the % error. and our % error is
19%.
My data does not support the law of definite proportions because our data are far away from the best fit line which has a slope of y= 0.51*x-0.012. But our class data works because the r2=0.594 tells us that class data is almost as one with is really close to the best-fit line. Some points that could be ignored are the negative point because you can't have a negative mass. In this lab, we had 19% of error. Some of the things that could have affected the results was our piece of Mg wouldn't start. Instead of leaving it in the container we put it into the bunsen burner flame to get it started once it started we put it back into the container. The error was that some of the mass could have escaped during that time. Another thing that could lead to our error was once we got the Mg to go and it was almost cool we took it off of the stand and dropped on the counter. The error was that our mass was not quite right because we might drop some of the Mg masses before we weighted it. The third possible source of error is our mass and measurements. Because we dropped the crucible we could have lots some of our products which would affect the mass. To conclude, some of the errors that could have affected our results.