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How would you determine yield of the main product if 0.29 g of crcl3-6h2o is used, 1 g of urea is used and 0.8 ml of acac is used. balanced reaction: 2 CrCl3.6H2O + 3 H2NCONH2 + 6 CH3COCH2COCH3 → 2 [cr(ch3cochcoch3)3] + 6 NH4Cl + 12 H2O
Accepted Answer
To determine the yield of the main product, [Cr(CH3COCHCOCH3)3], you need to follow these steps:
1. Identify the Limiting Reactant: Calculate the moles of each reactant using their molar masses:
CrCl3.6H2O: 0.29 g / (266.45 g/mol) = 0.00109 mol
H2NCONH2 (urea): 1 g / (60.06 g/mol) = 0.0167 mol
CH3COCH2COCH3 (acetylacetone): 0.8 mL
(1.02 g/mL) / (100.12 g/mol) = 0.00816 mol
Determine the limiting reactant by comparing the mole ratios in the balanced equation to the actual mole amounts. The reactant with the smallest ratio to its stoichiometric coefficient is the limiting reactant. For example, if the ratio of CrCl3.6H2O to its coefficient of 2 is smaller than the ratios for the other reactants, then CrCl3.6H2O is the limiting reactant.
2. Calculate Theoretical Yield: Using the moles of the limiting reactant and the stoichiometry of the balanced equation, calculate the theoretical yield of [Cr(CH3COCHCOCH3)3] in moles and then convert to grams using its molar mass.
3. Determine Actual Yield: You will need to perform the experiment to obtain the actual yield of the product. This is the amount of [Cr(CH3COCHCOCH3)3] you actually obtain after the reaction is complete.
4. Calculate Percent Yield: Divide the actual yield by the theoretical yield and multiply by 100%.
Percent Yield = (Actual Yield / Theoretical Yield)
100%
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