Answer to Question #154204 in General Chemistry for Sage Topaz

Question

Ethylene Glycol is used in automobile antifreeze and preparation of polyester fiber. Ethylene glycol is produced in the following reaction:

C₂H₂O  + H₂O ----> C₂H₆O₂  

If 90 g of water are used completely in the reaction, how many moles of ethylene glycol are produced? How many grams is this equivalent to?

Answer 1

Assuming that your equation is wrong (that you meant C₂H₄O and not C₂H₂O as the reagent).

Because Ethylene glycol is produced from ethene via an intermediate ethylene oxide (C₂H₄O). It is ethylene oxide that is reacted with water to form ethylene glycol as shown below;

C₂H₄O + H₂O $\implies$ C₂H₆O₂

Mole ratio of all species involved is 1:1:1

Moles of water in 90g

$Moles = \dfrac{mass}{MM} = \dfrac{90g}{18g/mol} = 5mol$

Moles of ethylene glycol according to the equation

Moles of C₂H₆O₂ =$\dfrac{1}{1}x 5mol = 5 mol$

Mass of C₂H₆O₂ = Moles x MM of C₂H₆O₂

= 5 mol x 62 g/mol

= 310g