Atom economy

Calculate the atom economy of a reaction as the molar mass of the desired product divided by the total molar mass of all products, explain why it matters in green chemistry, and distinguish it from percentage yield.

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Which route to chloroethane has an atom economy of 100 %? A. $\ce{C2H5OH + PCl5 -> C2H5Cl + POCl3 + HCl}$ B. $\ce{C2H6 + Cl2 -> C2H5Cl + HCl}$ C. $\ce{C2H5OH + HCl -> C2H5Cl + H2O}$ D. $\ce{C2H4 + HCl -> C2H5Cl}$

One route to 2-bromopropane is the substitution of propane by bromine in ultraviolet light. $\ce{C3H8(g) + Br2(g) -> C3H7Br(g) + HBr(g)}$ ( $\ce{C3H8}$ = 44.11 $\mathrm{g\,mol^{-1}}$ , $\ce{Br2}$ = 159.80 $\mathrm{g\,mol^{-1}}$ , $\ce{C3H7Br}$ = 123.00…

For the overall reaction shown above, calculate the atom economy of this route from propane and ethane to propyl ethanoate. Use sections 1 and 7 of the data booklet.

(i) If the reaction has a percentage yield of 80 %, calculate the mass, in g, of benzene that would be produced from 2.0 kg of cyclohexane. (ii) Calculate the atom economy for this reaction, as a percentage.

Butan-2-ol reacts with octadecanoic (stearic) acid to form an ester that is used as a lubricant. $\ce{C17H35COOH(l) + CH3CH(OH)CH2CH3(l) <=> C17H35COOCH(CH3)CH2CH3(l) + X(l)}$ (i) Identify the by-product X(l) and state the type of reaction taking place. (ii)…

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