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Diethyl ether is produced from ethanol according to the following equation: 2CH3CH2OH(l) → CH3CH2OCH2CH3(l) + H2O(l) Calculate the percent yield if 65.2 g of ethanol reacts to produce 17.2 g of ether.

User Bmatovu
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1 Answer

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Answer : The percent yield is, 32.79 %

Explanation :

First we have to calculate the moles of
CH_3CH_2OH.


\text{Moles of }CH_3CH_2OH=\frac{\text{Mass of }CH_3CH_2OH}{\text{Molar mass of }CH_3CH_2OH}=(65.2g)/(46.07g/mole)=1.415mole

Now we have to calculate the moles of
CH_3CH_2OCH_2CH_3

The balanced chemical reaction will be,


2CH_3CH_2OH(l)\rightarrow CH_3CH_2OCH_2CH_3(l)+H_2O(l)

From the balanced reaction, we conclude that

As, 2 moles of
CH_3CH_2OH react to give 1 mole of
CH_3CH_2OCH_2CH_3

So, 1.415 moles of
CH_3CH_2OH react to give
(1.415)/(2)=0.7075 mole of
CH_3CH_2OCH_2CH_3

Now we have to calculate the mass of
CH_3CH_2OCH_2CH_3


\text{Mass of ether}=\text{Moles of ether}* \text{Molar mass of ether}


\text{Mass of }ether=(0.7075mole)* (74.12g/mole)=52.44g

The theoretical yield of ether,
CH_3CH_2OCH_2CH_3 = 52.44 g

Now we have to calculate the percent yield of
CH_3CH_2OCH_2CH_3


\%\text{ yield of ether}=\frac{\text{Actual yield of ether}}{\text{Theoretical yield of ether}}* 100=(17.2g)/(52.44g)* 100=32.79\%

Therefore, the percent yield is, 32.79 %

User Md Mahbubur Rahman
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