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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. actually calculate
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:
CrCl3.6H2O: (0.29 g / 266.45 g/mol) = 0.00109 mol
Urea (H2NCONH2): (1 g / 60.06 g/mol) = 0.0167 mol
Acac (CH3COCH2COCH3): (0.8 mL
1.025 g/mL / 100.12 g/mol) = 0.0082 mol
Determine the limiting reactant by comparing the mole ratios to the stoichiometric coefficients in the balanced equation. The reactant with the smallest mole ratio to its stoichiometric coefficient is the limiting reactant. In this case, it's CrCl3.6H2O.
2. Calculate the Theoretical Yield:
Use the mole ratio from the balanced equation between the limiting reactant (CrCl3.6H2O) and the main product ([Cr(CH3COCHCOCH3)3]) to calculate the theoretical yield of the product in moles.
Theoretical yield (mol): 0.00109 mol CrCl3.6H2O
(2 mol [Cr(CH3COCHCOCH3)3] / 2 mol CrCl3.6H2O) = 0.00109 mol [Cr(CH3COCHCOCH3)3]
Convert the theoretical yield from moles to grams.
Theoretical yield (g): 0.00109 mol
490.42 g/mol = 0.534 g
3. Determine the Actual Yield:
The actual yield is the amount of product you obtain in the experiment. You would need to perform the reaction and measure the mass of the isolated product to get the actual yield.
4. Calculate the Percentage Yield:
Percentage Yield = (Actual Yield / Theoretical Yield)
100%
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