Maleic anhydride, C4 H2 O3, can be produced by the oxidation...

Maleic anhydride, $\mathrm{C}_{4} \mathrm{H}_{2} \mathrm{O}_{3},$ can be produced by the oxidation of benzene (Study Question 141 ). It can also be produced from the oxidation of butene. (a) What is the \% atom economy for the synthesis of maleic anhydride from butene by this reaction? (b) If $1.02 \mathrm{kg}$ of maleic anhydride is produced from exactly $1.00 \mathrm{kg}$ of butene, what is the percent yield of the anhydride? What mass of the byproduct $\mathrm{H}_{2} \mathrm{O}$ is also produced?

Maleic anhydride, $\mathrm{C}_{4} \mathrm{H}_{2} \mathrm{O}_{3},$ can be produced by the oxidation of benzene (Study Question 141 ). It can also be produced from the oxidation of butene.
(a) What is the \% atom economy for the synthesis of maleic anhydride from butene by this reaction?
(b) If $1.02 \mathrm{kg}$ of maleic anhydride is produced from exactly $1.00 \mathrm{kg}$ of butene, what is the percent yield of the anhydride? What mass of the byproduct $\mathrm{H}_{2} \mathrm{O}$ is also produced?

Key Concepts

Conservation of Mass

The conservation of mass principle states that the total mass of the reactants in a chemical reaction must equal the total mass of the products. This concept is applied during the stoichiometric calculations to ensure that mass is neither created nor destroyed during a chemical reaction, and it is critical when determining the mass of byproducts formed alongside the desired product.

Stoichiometry

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. It requires balancing the chemical equation and converting between mass, moles, and molecular quantities using molar masses. This concept is fundamental in calculating theoretical yields, the ratio of byproducts, and in ensuring mass conservation in any chemical reaction.

Percent Yield

Percent yield measures the efficiency of a reaction by comparing the actual amount of product obtained to the theoretical amount predicted by stoichiometric calculations. It is calculated by taking the ratio of the actual yield to the theoretical yield, then multiplying by 100. This concept is vital for assessing the practical performance of a chemical synthesis and identifying any losses due to side reactions, incomplete reactions, or practical inefficiencies.

Atom Economy

Atom economy is a measure of how efficiently a chemical reaction converts reactants into the final desired product. It is calculated by dividing the molecular weight of the desired product by the total molecular weight of all reactants that become part of the product, multiplied by 100 to get a percentage. This concept is crucial in green chemistry as it helps evaluate how much waste is generated in a reaction relative to the product formed.

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