53.0 g of silver (1) nitrate reacts according to the reaction shown below: AgNO3 + KCI — AGCI + KNO3
Find the theoretical yield of AgCl. If the amount of AgCl actually produced is 38.5 grams,
what is the percent yield of the experiment?

Percent yield = 86.09%

Theoretical yield of AgCl = 44.72 g

Explanation:

Given data:

Mass of silver(1) nitrate = 53.0 g

Actual yield of AgCl = 38.5 g

Theoretical yield of AgCl = ?

Percent yield = ?

Solution:

Chemical equation:

AgNO₃ + KCl    →   AgCl + KNO₃

Number of moles of AgNO₃:

Number of moles = mass/molar mass

Number of moles = 53.0 g/ 169.87 g/mol

Number of moles = 0.312 mol

now we will compare the moles of AgNO₃ and AgCl

               AgNO₃         :           AgCl

                   1               :                1

                0.312          :           0.312

Theoretical yield of AgCl:

Mass = number of moles × molar mass

Mass = 0.312 mol × 143.32 g/mol

Mass = 44.72 g

Percent yield:

Percent yield = (actual yield / theoretical yield) × 100

Percent yield = ( 38.5 g / 44.72 g ) × 100

Percent yield = 86.09%

< > according to newton's third law of motion, forces always act in equal but opposite pairs. another way of saying this is for every action, there is an equal but opposite reaction.< >