Which of the following below explain why the alcohol is used in excess in this reaction. Note that there may be more than one answer.

The alcohol is used in excess to make the reaction mixture soluble in ether during the extraction phase.

The alcohol is used in excess to remove all of the protons from the carboxylic acid.

This is a reversible reaction and adding excess alcohol drives the reaction towards the reactants.

This is a reversible reaction and adding excess alcohol drives the reaction towards the products.

There is no need to add excess alcohol, excess ester should be added.

The alcohol is less expensive and easier to remove from the product mixture than the carboxylic acid, but an excess of either would help in this reaction.

Excess alcohol completely neutralizes the sulfuric acid and makes the reaction safer.

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1.Which of the following statements are true about sulfuricacid's role in the esterification reaction. Note thatthere may be more than one correct answer.

		sulfuric acid is added to lower the boiling point of thereaction mixture.
		sulfuric acid protonates the carboxylic acid in the first stepof the reaction mechanism
		sulfuric acid is used to ensure the alcohol will dissolve inether
		sulfuric acid protonates the ester in the first step of thereaction mechanism
		sulfuric acid protonates the alcohol in the first step of thereaction mechanism
		sulfuric acid reduces the concentration of OH^- andslows the reverse reaction.
		sulfuric acid is used to ensure the carboxylic acid willdissolve in ether
		sulfuric acid is added to react with excess sodium bicarbonatein the first step of the reaction
		sulfuric acid acts as a catalyst for the reaction

2.Which of the following below explain why the alcohol is usedin excess in this reaction. Note that there may be morethan one answer.

		This is a reversible reaction and adding excess alcohol drivesthe reaction towards the products.
		This is a reversible reaction and adding excess alcohol drivesthe reaction towards the reactants.
		There is no need to add excess alcohol, excess ester should beadded.
		The alcohol is used in excess to make the reaction mixturesoluble in ether during the extraction phase.
		The alcohol is used in excess to remove all of the protons fromthe carboxylic acid.
		Excess alcohol completely neutralizes the sulfuric acid andmakes the reaction safer.
		The alcohol is less expensive and easier to remove from theproduct mixture than the carboxylic acid, but an excess of eitherwould help in this reaction.

3.Why is a sodium bicarbonate solution used to extract the ether(organic) layer. Note that there may be more than onecorrect answer.

		sodium bicarbonate reacts with the ester to make it soluble inwater.
		sodium bicarbonate should not be added, sulfuric acid should beadded during the extraction.
		sodium bicarbonate reacts with any leftover sulfuric acid toform a salt that is INsoluble in the organic layer.
		sodium bicarbonate reacts with the alcohol to make it solublein water.
		sodium bicarbonate is added because it is less expensive thanadding hydrochloric acid.
		sodium bicarbonate reacts with any leftover carboxylic acid toform a salt that is INsoluble in the organic layer.
		sodium bicarbonate reacts with any leftover carboxylic acid toform a salt that is soluble in the organic layer.
		sodium bicarbonate is used to react with ether and make theyield of the ester product greater.
		sodium bicarbonate reacts with any leftover sulfuric acid toform a salt that is soluble in the organic layer.

1.Which of the following statements are true about sulfuricacid's role in the esterification reaction. Note thatthere may be more than one correct answer.

		sulfuric acid is added to lower the boiling pointof the reaction mixture.
		sulfuric acid protonates the carboxylic acid inthe first step of the reaction mechanism
		sulfuric acid is used to ensure the alcohol willdissolve in ether
		sulfuric acid protonates the ester in the firststep of the reaction mechanism
		sulfuric acid protonates the alcohol in the firststep of the reaction mechanism
		sulfuric acid reduces the concentration ofOH^- and slows the reverse reaction.
		sulfuric acid is used to ensure the carboxylicacid will dissolve in ether
		sulfuric acid is added to react with excess sodiumbicarbonate in the first step of the reaction
		sulfuric acid acts as a catalyst for thereaction

2.Which of the following below explain why thealcohol is used in excess in this reaction. Note thatthere may be more than one answer.

		This is a reversible reaction and adding excessalcohol drives the reaction towards the products.
		This is a reversible reaction and adding excessalcohol drives the reaction towards the reactants.
		There is no need to add excess alcohol, excessester should be added.
		The alcohol is used in excess to make the reactionmixture soluble in ether during the extraction phase.
		The alcohol is used in excess to remove all of theprotons from the carboxylic acid.
		Excess alcohol completely neutralizes the sulfuricacid and makes the reaction safer.
		The alcohol is less expensive and easier to removefrom the product mixture than the carboxylic acid, but an excess ofeither would help in this reaction.

3.Why is a sodium bicarbonate solution used to extract the ether(organic) layer. Note that there may be more than onecorrect answer.

		sodium bicarbonate reacts with the ester to makeit soluble in water.
		sodium bicarbonate should not be added, sulfuricacid should be added during the extraction.
		sodium bicarbonate reacts with any leftoversulfuric acid to form a salt that is INsoluble in the organiclayer.
		sodium bicarbonate reacts with the alcohol to makeit soluble in water.
		sodium bicarbonate is added because it is lessexpensive than adding hydrochloric acid.
		sodium bicarbonate reacts with any leftovercarboxylic acid to form a salt that is INsoluble in the organiclayer.
		sodium bicarbonate reacts with any leftovercarboxylic acid to form a salt that is soluble in the organiclayer.
		sodium bicarbonate is used to react with ether andmake the yield of the ester product greater.
		sodium bicarbonate reacts with any leftoversulfuric acid to form a salt that is soluble in the organiclayer.