When 38.21 g of pure copper reacts with 192.83g of iodine, 190.83g of a compound containing only
copper and iodine result. 40.21g of iodine remain when the reaction is complete.
a. Do these results support the Law of Conservation of Mass? Explain.
b.does this compund obey the laws of multiple porportions? Explain.
im not sure exactly how to answer this question, would the 40.21 be subtracted from the 190.83?
mass reactants:
38.21 + 192.83 = 231.04 g.
mass products + left over:
190.83 + 40.21 = 231.04 g.
Looks to me like mass reacts equals mass product plus the left over so mass is conserved.
To answer the question, let's break it down step by step:
a. Does the result support the Law of Conservation of Mass? The Law of Conservation of Mass states that in a chemical reaction, mass is neither created nor destroyed; it is conserved. To verify if the law is supported, we need to compare the total mass of reactants with the total mass of products.
In this case, the total mass of reactants is 38.21g (copper) + 192.83g (iodine) = 231.04g.
The total mass of products is 190.83g (compound) + 40.21g (remaining iodine) = 231.04g.
As we can see, the total mass of reactants is indeed equal to the total mass of products, supporting the Law of Conservation of Mass. So, the answer to part a is yes.
b. Does this compound obey the laws of multiple proportions? The law of multiple proportions states that when two elements combine to form different compounds, the ratio of the masses of one element that combine with a fixed mass of the other element is always a ratio of small whole numbers.
In this case, to determine if the compound follows the law of multiple proportions, we need to examine the ratio of iodine to copper in the compounds involved.
The initial reactants contain 192.83g of iodine and 38.21g of copper, which gives a ratio of 192.83g / 38.21g = 5.05 (approx).
The resulting compound contains 190.83g of the compound with 40.21g of remaining iodine. If we subtract the amount of remaining iodine from the total compound, we get 190.83g - 40.21g = 150.62g of compound.
Therefore, the ratio of iodine to copper in the compound is 150.62g / 38.21g = 3.94 (approx).
Since the ratio of iodine to copper in the resulting compound is not a simple ratio of small whole numbers, it does not follow the law of multiple proportions.
So, the answer to part b is no.
To summarize, the results support the Law of Conservation of Mass but do not adhere to the laws of multiple proportions.