Answer:
Explanation:
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In this case, when we want to balance chemical reactions such as in this case, the idea is to equal to number of atoms of each element at each side of the equation according to the lay of conservation of mass, just as shown below:
Because we have four phosphorous and ten oxygen atoms at each side.
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Answer:
A. 10.0 grams of ethyl butyrate would be synthesized.
B. 57.5% was the percent yield.
C. 7.80 grams of ethyl butyrate would be produced from 7.60 g of butanoic acid.
Explanation:
A
Moles of butanoic acid =
According to reaction ,1 mole of butanoic acid gives 1 mol of ethyl butyrate,then 0.08636 mol of butanoic acid will give :
of ethyl butyrate
Mass of 0.08636 moles of ethyl butyrate =
0.08636 mol × 116 g/mol = 10.0 g
Theoretical yield = 10.0 g
Experimental yield = ?
Percentage yield of the reaction = 100%
Experimental yield = 10.0 g
10.0 grams of ethyl butyrate would be synthesized.
B
Theoretical yield of ethyl butyrate = 10.0 g
Experimental yield ethyl butyrate = 5.75 g
Percentage yield of the reaction = ?
57.5% was the percent yield.
C
Moles of butanoic acid =
According to reaction ,1 mole of butanoic acid gives 1 mol of ethyl butyrate,then 0.08636 mol of butanoic acid will give :
of ethyl butyrate
Mass of 0.08636 moles of ethyl butyrate =
0.08636 mol × 116 g/mol = 10.0 g
Theoretical yield = 10.0 g
Experimental yield = ?
Percentage yield of the reaction = 78.0%
Experimental yield = 7.80 g
7.80 grams of ethyl butyrate would be produced from 7.60 g of butanoic acid.