Ethyl butyrate, ch3ch2ch2co2ch2ch3, is an artificial fruit flavor commonly used in the food industry for such flavors as orange and pineapple. its fragrance and taste are often associated with fresh orange juice, and thus it is most commonly used as orange flavoring. it can be produced by the reaction of butanoic acid with ethanol in the presence of an acid catalyst (h+): ch3ch2ch2co2h(l) + ch2ch3oh(l) ⟶ ch3ch2ch2co2ch2ch3(l) + h2o(l) now lets say that you discover a more efficient catalyst that can produce ethyl butyrate with a 79.1 % yield. how many grams of ethyl butyrate would be produced from 13.58 g of butanoic acid and excess ethanol?

             14.15 g of Ethyl Butyrate

Solution:

The Balance Chemical Equation is as follow;

           Butanoic Acid  +  Ethanol    →    Ethyl Butyrate  +  Water

Molar Mass of Butanoic Acid  =  88.11 g.mol⁻¹

Molar Mass of Ethanol  =  46.07 g.mol⁻¹

Molar Mass of Ethyl Butyrate  =  116.16 g.mol⁻¹

Molar Mass of Water  =  18.01 g.mol⁻¹

Step 1: Calculating Theoretical Yield:

According to Equation,

           88.11 g (1 mol) Butanoic Acid forms  =  116.16 g (1 mol) Ethyl Butyrate

So,

                 13.58 g Butanoic Acid will form  =  X g of Ethyl Butyrate

Solving for X,

                     X  =  (13.58 g × 116.16 g) ÷ 88.11 g

                     X  =  17.90 g

                     Theoretical Yield  =  17.90 g

Step 2: Calculating Actual Yield:

As,

                     %age Yield  =  Actual Yield ÷ Theoretical Yield × 100

Solving for Actual Yield,

                      Actual Yield  =  %age Yield × Theoretical Yield ÷ 100

Putting Values,

                      Actual Yield  =  79.1 × 17.90 ÷ 100

                      Actual Yield =  14.15 g of Ethyl Butyrate

the correct answer would be d. hope this !