When 38.21 g of pure copper reacts with 192.83g of iodine, 190.83g of a compound

Question

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. Do these results support the Law of Conservation of Mass? Explain Is this compound the same as the compounds in from Problem 2.19? Even if you know- about them, you may not use moles to solve this problem. If your answer to part b was that this is a different compound, prove that the data obeys the Law of Multiple proportions.

Explanation / Answer

6a) The Law of Conservation of Mass states that mass is indestructible, i.e, it can neither be created nor be destroyed. What this essentially means in the given context is that the mass of the reactants before the reaction and the mass of the products after the reaction must be the same.

We started with 38.21 gm of pure copper and 192.83 gm of iodine. The combined mass of the reactants before the reaction is (38.21 + 192.83) gm = 231.04 gm.

We obtained a product containing only copper and iodine and the mass of the product obtained is 190.83 gm. 40.21 gm of iodine was left unreacted. Therefore, the combined mass of the product and the excess reactant after the reaction is (190.83 + 40.21) gm = 231.04 gm.

We therefore see that the mass of the materials before and after the reaction remains the same; this proves that the Law of Conservation of Mass is obeyed in this case.

b+c) I need to know the answer to Problem 2.19 or the problem itself to answer these two parts.

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