Question

When 500.0 g of water is decomposed by electrolysis and the yield of hydrogen is only 75.3%, how much hydrogen chloride can be made if the yield of hydrogen chloride in the second reaction is 69.8%? Oxygen and chlorine and in excess.

2H₂O → 2H₂ + O₂ 75.3 % yield
H₂ + Cl₂ → 2HCl 69.8% yield

Answer 1

The amount of hydrogen chloride that can be made is 1064 g

Why?

The two reactions are:

2H₂O → 2H₂ + O₂ 75.3 % yield

H₂ + Cl₂ → 2HCl 69.8% yield

We have to apply a big conversion factor to go from grams of water (The limiting reactant), to grams of HCl, the final product. We have to be very careful with the coefficients and percentage yields!

$500.0gH_2O*\frac{1moleH_2O}{18.01 gH_2O}*\frac{2 moles H_2}{2 moles H_2O}*\frac{2.015g H_2}{1 mole H_2}*\frac{75.3 actual g}{100 theoretical g}=42.12 g H_2$

$42.12H_2*\frac{1 mole H_2}{2.015gH_2}*\frac{2 moles HCl}{1 mole H_2}*\frac{36.46g}{1 mole HCl}*\frac{69.8 actualg}{100 theoreticalg} =1064gHCl$

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Answer 2

The amount of hydrogen chloride yield in the second reaction is 1065.7 g.

The two given reactions

• 2H₂O → 2H₂ + O₂ 75.3 % yield
• H₂ + Cl₂ → 2HCl 69.8% yield

The amount of hydrogen gas yield in the first reaction is calculated as follows;

$\frac{500 \ g\ H_2O}{18 \ g \ H_2O} \times (2 \ mol\ H_2) \times 0.753= 41.83 \ g \ H_2$

The amount of hydrogen chloride yield in the second reaction is calculated as follows;

$41.83 \ g \times (36.5 \ HCl) \times 0.698 = 1065.7 \ g \ HCl$

Thus, the amount of hydrogen chloride yield in the second reaction is 1065.7 g.

Learn more about hydrogen yield in electrolysis here: https://brainly.com/question/10692990