Ether, (C_2H_5)_2O. Is an organic compound which was used as a cheap and effecti

Question

Ether, (C_2H_5)_2O. Is an organic compound which was used as a cheap and effective for many years. It has now been replaced by safer and more effective medications. . he prepared from ethanol. C_2H_5OH, according to the balanced equation below; using a strong acid as a catalyst. Since the catalyst only facilitates the reaction, it is not men one the balanced equation. 2 C_2H_5OH rightarrow (C_2H_5)_2O + H_2O Ether has a density of 0.7134 g/mL. Ethanol has a density of 0.7894 g/mL. Calculate the % yield of this reaction if 1.250 L of ether is produced from the reaction ol 1.550 L ethanol. Round your answer to the correct number of significant figures.

Explanation / Answer

The reaction is:

2 C2H5OH  --------> (C2H5)2O

According to stoichiometry 2 moles of ethanol produce 1 mole of ether.

First we have to calculate mass of ethanol using density and considering 1.550L = 1,550ml:

mass of ethanol= densityxVolume = (0.7894g/ml)(1,550ml) = 1,224 g of ethanol

moles of ethanol= mass/molar mass = 1,224g/46.068g/mol =26.57moles of ethanol

In tables : molar mass ethanol= 46.068g/mol

According to stoichiometry:

moles of ether produced= 26.57moles(1mmol ether/2 moles alcohol) = 13.29 moles eher

molar mass of ether(In tables) = 74.12g/mol

mass of ether= (13.29moles)(74.12g/mol) = 985.1g ether (In theory).

You really got:

mass of ether=( density)(volume)= (0.7134g/ml)(1,250ml) = 891.8g of ether

% yield of this reaction:

% yield = (mass experimental)(100)/mass in theory

%yield= (891.8g)(100)/(985.1) = 90.53%

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