Answer:
2 water + sugar + lemon juice → 4 lemonade
Calculating the moles of water in 946.36 g of water=\frac{946.36 g}{236.59 g/mol}=4 mol=
236.59g/mol
946.36g
=4mol
Calculating the moles of sugar in 196.86 g of sugar=\frac{196.86 g}{225 g/mol}=0.8749 mol=
225g/mol
196.86g
=0.8749mol
Calculating the moles of lemon juice in 193.37 g of lemon juice=\frac{193.37 g}{257.83 g/mol}=0.7499 mol=
257.83g/mol
193.37g
=0.7499mol
Calculating the moles of lemonade in 2050.25 g of lemonade=\frac{2050.25 g}{719.42 g/mol}=2.8498 mol=
719.42g/mol
2050.25g
=2.8498mol
It is apparent that the amount of lemon juice limits the reaction.
Consequently, we will base the reaction's completion on the quantity of lemon juice.
1 mole of lemon juice reacts with 2 moles of water, therefore, 0.7499 mol of lemon juice will react with:
\frac{2}{1}\times 0.7499 mol = 1.4998 mol
1
2
×0.7499mol=1.4998mol of water
Mass of water utilized = 1.4998 mol × 236.59 g/mol=354.8376 g
Unused water = 946.36 g - 354.8376 g =591.5223 g
1 mole of lemon juice reacts with 1 mole of sugar, thus 0.7499 mol of lemon juice will react with:
\frac{1}{1}\times 0.7499 mol = 0.7499 mol
1
1
×0.7499mol=0.7499mol of sugar
Mass of sugar consumed = 0.7499 mol × 225 g/mol = 168.7275 g
Excess sugar = 196.86 g - 168.7275 g
1 mole of lemon juice results in 4 moles of lemonade.
Hence, 0.7499 mol of lemon juice will produce:
\frac{4}{1}\times 0.7499 mol=2.996 mol
1
4
×0.7499mol=2.996mol of lemonade
The mass of lemonade yielded = 2.996 mol × 719.42 g/mol = 2157.9722 g
Theoretical production of lemonade = 2157.9722 g
Actual yield of lemonade = 2050.25 g
Calculating the percentage yield of lemonade:
\frac{\text{Actual yield}}{\text{theoretical yield}}\times 100
theoretical yield
Actual yield
× 100
\frac{2050.25 g}{2157.9722 g}\times 100=95.00\%
2157.9722g
2050.25g
× 100=95.00%