How do I determine/compare the theoretical calculations to my experimental resul

Question

How do I determine/compare the theoretical calculations to my experimental results and then state whether Equation 1 or 2 represents the reaction that actually occurred? 1) Fe(s) + CuSO4 (aq) ! FeSO4 (aq) + Cu(s) Fe(s) + Cu+2(aq) ! Fe+2(aq) + Cu(s) (2) 2Fe(s) + 3CuSO4 (aq) ! Fe2(SO4)3 (aq) + 3Cu(s) 2Fe(s) + 3Cu+2(aq) ! 2Fe+3(aq) + 3Cu(s) An

Explanation / Answer

This type of reaction, in which one metal "displaces" another from a solution of one of its salts, is known as a single substitution reaction. A metal capable of displacing another from a solution of one of its salts is said to be "more active" than the displaced metal. In this experiment, iron is more active than copper. Iron forms 2 types of ions, namely Fe+2 and Fe+3. We shall use stoichiometric principles to determine which of these ions is formed in the reaction between iron and copper (II) sulfate solution. If Fe+2 is formed, then equation (1) is correct, while equation (2) is correct if Fe+3 is formed. We are using sulfate (SO4 2-) the oxidation state of Fe is 2+. Fe(s) + Cu2+(aq) ---> Fe2+(aq) + Cu(s) We know the molar ratios and this is done to find out No. of moles we have of Fe , which will also equal the amount of moles of Cu since the ratio is 1:1. 1.0 g Fe x (1 mol / 55.845 g) = 0.0179 mol Fe So, we need 0.0179 mol of Cu2+ solution to complete the reaction. The equation for molarity: molarity = mol / volume in liters. 1.0 M = 0.0179 mol / V V = 0.0179 mol / 1 V = 0.0179 liters Now for 2Fe(s) + 3Cu+2(aq) ---> 2Fe+3(aq) + 3Cu(s) We know the molar ratios and this is done to find out No. of moles we have of Fe , which is the amount of moles of Cu since the ratio is 2:3. Similarly doing all the calculations we can solve it.We shall use stoichiometric principles to determine which of these ions is formed in the reaction between iron and copper (II) sulfate solution.

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