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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
`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.
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