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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=

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onyebuchinnaji

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

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