Conclusion Results To determine the limiting reagent, the mole ratios are compared to the balanced chemical equation: 2CoCO_3 (s)+6(acacH)(l)+H_2 O_(2 ) (aq) 2Co(acac)_3 (s)+4H_2 O(l)+2CO_2 (aq) 8 Which gives the ratio 2 moles CoCO3 : 6 moles acac : 1 mole H2O2.8 The reagents were measured at 2.5 g Co(II)CO3, 20.0 mL acetalacetone, and 30.0 mL of 10% hydrogen peroxide (H2O2). ... A mole ratio comparison determined CoCO3 was the limiting reagent, which lead to a theoretical yield calculation of 7.518g Co(acac)3. ...

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In the calculations for the first product, the molecular weight was multiplied by 0.03 grams, because furan was the limiting agent. ... Since furan was the limiting reagent, if furan was measured incorrectly, then the amount of product formed would also be affected. ...

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Results 1) Calculation of moles and the limiting reactant of the starting materials: 10mL X (0.810g/1mL) X (1mol/74.12g) = 0.109moles of n-Butyl alcohol (limiting reagent) 17.0g X (1mol/102.89g) = 0.165moles of sodium bromide 14.0mL X (1L/1000mL) X (18.4mol/1L) = 0.2576 moles of Sulfuric acid 2) Calculation of theoretical yield: 10.0mL 1-butanol X (0.810g/1mL) X (1mol/74.12g) X (137.03g/1mol) = 14.97g n-Butyl bromide 3) Calculation of percent yield: (11.09g n-Butyl bromide collected/14.97g theoretical amount) X 100 = 74.1% yield Discussion The theoretical yield for the reaction was ...

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