63. Ethanol is produced industrially by reacting ethylene gas with water. The balanced equation for this reaction is: C2H4(g) + H₂O(/) → C₂H5OH() If water is present in excess, how many grams of ethanol can be produced from 8.0 g of ethylene?

63. Ethanol is produced industrially by reacting ethylene gas with water. The balanced equation for this reaction is: C2H4(g) + H₂O(/) → C₂H5OH() If water is present in excess, how many grams of ethanol can be produced from 8.0 g of ethylene?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.44PAE: 4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of...

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Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

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63. Ethanol is produced industrially by reacting ethylene gas with water. The balanced
equation for this reaction is:
C2H4(g) + H₂O(/) → C₂H5OH()
If water is present in excess, how many grams of ethanol can be produced from 8.0
g of ethylene?

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