Percentage yield and atom economy
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Intros
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Examples
Lessons
- Find the atom economy and percentage yield of chemical reactions.
Water can be produced by reaction of hydrogen and oxygen gas according to this equation:
2 HO→2 HO - Find the atom economy and percentage yield of chemical reactions.
The reaction to make iron metal by reduction uses carbon. CO is an unwanted side-product. The reaction is as follows:
2 FeO3 C→3 CO4 Fe - What is the atom economy of this reaction?
- 280 g of FeO was used in this reaction and 104 g of Fe metal was collected. Calculate the theoretical yield and then the percentage yield of this reaction.
- This reaction was done again and a percentage yield of 90% was achieved this time. If 250 g of Fe was collected this time, how much FeO was used up?
- Compare the viability of two reactions by finding the atom economy and percentage yield.
Magnesium reacts with hydrochloric acid as shown in the following equation:
Mg2 HCl→MgClH - If this reaction was performed to make hydrogen gas, what would be the atom economy?
- 55 g of Mg metal was used in this reaction with HCl in excess. Only 4.21 g of H gas was produced from this reaction. What is the percentage yield of this reaction?
- Hydrogen gas could also be made by electrolysis of water, in the following reaction:
2 HO→2 HO
Find the atom economy of this reaction. Is it a better or worse way to make hydrogen than reacting magnesium with hydrochloric acid?