Explore Westonci.ca, the leading Q&A site where experts provide accurate and helpful answers to all your questions. Join our Q&A platform and connect with professionals ready to provide precise answers to your questions in various areas. Get immediate and reliable solutions to your questions from a community of experienced professionals on our platform.

Which of the following is the correct set-up for the problem: How many grams of water will be produced from 3.2 moles of oxygen and an excess of C2H4?​

Which Of The Following Is The Correct Setup For The Problem How Many Grams Of Water Will Be Produced From 32 Moles Of Oxygen And An Excess Of C2H4 class=

Sagot :

Option C is the correct set of the problem for mass of water produced by 3.2 moles of oxygen and an excess ethene.

Reaction between oxygen and ethene

Ethene (C2H4) burns in the presence of oxygen (O2) to form carbon dioxide (CO2) and water (H2O) along with the evolution of heat and light.

C₂H₄  + 3O₂   ----- > 2CO₂ + 2H₂O

from the equation above;

3 moles of O₂ ---------> 2(18 g) of water

3.5 moles of O₂ ----------> x

[tex]x = 3.2 \times [\frac{2 \ moles \ H_2O}{3 \ moles \ O_2} ] \times[ \frac{18.02 \ g \ H_2O}{1 \ mole \ H_2O} ][/tex]

Thus, option C is the correct set of the problem for mass of water produced by 3.2 moles of oxygen and an excess ethene.

Learn more about reaction of ethene here: https://brainly.com/question/4282233

#SPJ1

Thank you for choosing our platform. We're dedicated to providing the best answers for all your questions. Visit us again. We appreciate your time. Please revisit us for more reliable answers to any questions you may have. We're glad you visited Westonci.ca. Return anytime for updated answers from our knowledgeable team.