Zinc reacts with hydrochloric acid in a single replacement reaction. If 2.62 grams of zinc react with 3.65 grams of hydrochloric acid, then how many grams of hydrogen are actually produced if the...

Zinc reacts with hydrochloric acid in a single replacement reaction. If 2.62 grams of zinc react with 3.65 grams of hydrochloric acid, then how many grams of hydrogen are actually produced if the reaction has a 93% yield?

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jerichorayel | College Teacher | (Level 2) Senior Educator

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First, we have to make the balanced chemical equation for this reaction.

`Zn + 2 HCl -> ZnCl_2 + H_2`

Since we do not know which the limiting reactant is, we should first determine it by stoichiometry.

`2.62 grams Zn * (1 mol e Zn)/(65.38 grams Zn) * (1 mol e H_2)/(1 mol e Zn)`

`= 0.04007 mol es H_2`

 

`3.65 grams HCl * (1 mol e HCl)/(36.46 grams) * (1 mol e H_2)/(2 mol es HCl)`

`= 0.05005 mol es H_2`

 

Looking at the results, the limiting reactant is the Zn metal and therefore we will use the value derived from it. 

Theoretical amount of H2 gas formed:

`0.04007 mol es H_2 * (2.016 grams H_2)/(1 mol e H_2)`

`= 0.0808 grams of H_2 is p r oduced` -> theoretical yield

 

Percentage yield:

`percent yield = (actual yield)/(theo retical yield) * 100`

`(percent yield)/100 =(actual yield)/(theo retical yield)`

`actual yield = (93)/(100) *0.0808 grams`

actual yield = 0.0751 grams of H2 were actually produced. 

Sources:

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