Question

The reaction between silver nitrate and zinc chloride is 95% effective. If 250 g of silver nitrate reacts with 250 g of zinc chloride, what will be the actual yield of the products?


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Answer 1

balanced chemical reaction

ZnCl2 + 2AgNO3------>Zn(NO3)2 + 2AgCl

given :

250 g of ZnCl2 and

250 g of AgNO3

no. of moles of ZnCl2 = given mass/ molecular mass= 250 / 136.315 = 1.834

no. of moles of AgNO3 = given mass/ molecular mass= 250 / 169.87= 1.472

according to the balanced chemical reaction

1 mole of ZnCl2 reacts with 2 moles of AgNO3

=> 1.834 moles of ZnCl2 reacts with 2*1.834 = 3.668 moles of AgNO3

but only 1.472 moles of AgNO3 is present

=> AgNO3 is the limiting agent

so 2 mole of AgNO3 produces 2 mole of AgCl

=> 1 mole of AgNO3 produces 2/2 = 1 mole of AgCl

=> 1.472 moles of AgNO3 produces 1*1.472 = 1.472 moles of AgCl

theoretical mass of AgCl proiduced = no. of moles * molecular mass = 1.472*143.32 = 210.97

actual mass of AgCl produced = theoretical mass * percentage yield = 210.97*0.95 = 200.4 g

2 mole of AgNO3 produces 1 mole of Zn(NO3)2

=> 1 mole of AgNO3 produces 1/2 = 0.5 mole of Zn(NO3)2

=> 1.472 moles of AgNO3 produces 0.5*1.472 = 0.736 moles of Zn(NO3)2

theoretical mass of Zn(NO3)2 proiduced = no. of moles * molecular mass = 0.736*189.36 = 139.369 g

actual mass of Zn(NO3)2 produced = theoretical mass * percentage yield = 139.369*0.95 = 132.4 g

yield of the products are

Zn(NO3)2 = 132.4 g

AgCl = 200.4 g