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Lab Report Chem 1

by: Isabell Notetaker

Lab Report Chem 1

Marketplace > DMACC - Ankeny Campus > Science > > Lab Report Chem 1
Isabell Notetaker
DMACC - Ankeny Campus
GPA 3.52

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This lab report is about finding how much water is in Magnesium Sulfate
General Chemistry 1
Class Notes
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This 2 page Class Notes was uploaded by Isabell Notetaker on Sunday September 25, 2016. The Class Notes belongs to at DMACC - Ankeny Campus taught by in Spring 2015. Since its upload, it has received 2 views. For similar materials see General Chemistry 1 in Science at DMACC - Ankeny Campus.

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Date Created: 09/25/16
Isabell Akers 9/24/15 Finding How Much Water is in MgSO 4 Introduction: The purpose of this lab was to find out how much water was in Magnesium sulfate (MgSO ), and the molar ratio of water to Magnesium sulfate. 4 Materials & Methods: - Crucible - Tongs - Methane gas - MgSO (4olid powder) - Bunsen burner - Stand - Clay triangle - Ring clamp - Sand bowl - Scale in grams First we weighed our crucible, its’ mass was 11.746g. Next, we measured out 2.000g of MgSO . Th4 MgSO was th4n placed into the crucible, and was heated over a Bunsen burner for 12 minutes. After time was up we placed the crucible in a sand bowl to cool down. When it was cool enough to touch we weighed the crucible again, its’ mass was 12.781g. Results: To find how much water was in MgSO we took4how many grams of MgSO we 4 started with and subtracted how much we had after heating it. In the beginning of the lab we had 2.000g of Magnesium sulfate, and at the end we calculated how much Magnesium sulfate we had by subtracting the crucible with MgSO from the 4 weight of the crucible that we weighed in the beginning. 12.781g – 11.746g = 1.035g of MgSO 4 Now that we know how much Magnesium sulfate we have, we took our beginning weight of MgSO minu4 how much we had at the end. This shows us how much H O 2as in the MgSO to sta4t with. 2.000g – 1.035g = 0.965g of H O 2 To find out how many moles of H O was2produced, in gas form, we needed to convert g to moles, but first we had to find the molecular mass of water. H = 1.008, O = 16.00 2(1.008) + (16.00) = 18.016g = H O mol2r mass Isabell Akers 9/24/15 Now that we have the molar mass of water, we need to find out how many moles of water there was in Magnesium sulfate. .965g of H 2 x 1 mole = .0536 moles of H O2 18.016g Now we need to find out how many moles of MgSO we have4 but first we had to find the molar mass. Mg= 24.3 g S= 32.1 O= 16.00 (24.3) + (32.1) + 4(16.00) = 120.38g Now we found how many moles of MgSO there w4s at the end of the lab. 1.035g x 1 mole = 0.0086 g MgSO 4 120.38g To find the mole ratio of water to Magnesium sulfate, we divided by MgSO by 4 water. .0536 moles of H O2 .0086 moles of MgSO = 6.43 The actual value for the ratio of water to MgSO in4this experiment is 7, we got 6.23. We calculated our percent error by taking the accepted value minus our value and divided by the accepted value and times one hundred to make a percentage. ( 7 – 6.23 ) / 7 = 0.11 x 100 = 11% error Discussion: This lab was about finding how much water was in Magnesium sulfate, and we found out how many grams, moles, and the molar ratio of MgSO to H O. 4he 2 lab did not come out as well as I had hoped. I thought that we would be able to have a lower percent error but that did not happen. Some things that could have affected the lab are; the flame of the Bunsen burner being to low, or not keeping it on the flame long enough.


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