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Lab: Stoichemetry Investigation- Testing the Stoichiometric Method

In this class we were presented with a problem: Does Stoichiometry accurately predict the mass of products produced in chemical reactions?

I was in a group of three along with Sherilyn and Christina.
Our prediction before we started or experiment was to first, find out the balanced chemical equation for this reaction: 2.00g of Strontium nitrate is dissolved in 50mL of water and then reacted with excess Copper (II) sulphate (3.00g). The product is a precipitate (Strontium sulphate and Copper (II) nitrate.
Our balanced equation was: Sr(NO₃)₂ + CuSO₄ ® SrSO₄ + CU(NO₃)₂
Secondly we had to find how much of Strontium sulphate would be produced from 2.00g of Strontium nitrate. Our answer was: 2.00g x 1 mol x ­1 x 183.7g
                                                                     211.6g   1     1 mol    = 1.74g of SrSO₄

In the beginning of the experiment we had to carefully measure about 3.00g of Copper (II) sulphate and 2.00g of Strontium nitrate and dissolve them in separate beakers of 50mL of water. We slowly poured the two solutions together and mixed it. After pouring the solutions we had to measure a filter paper and filter the solution. Once finished we dried the filter paper and waited till dried.

posted by chemistry11 @ 9:11 PM