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C₂H₄ + 3O₂ → 2CO₂ + 2H₂O If you start with 45.9 g of C₂H₄, and excess O₂, what mass of CO₂ will be produced?

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The mass of CO2 that would be produced is 144.03 g

From the equation of the reaction, the mole ratio of C2H4 input to CO2 produced is 1:2.

Recall that: mole = mass/molar mass

mole of 45.9 g C2H4 = 45.9/28.05

                                     = 1.6364 moles

Thus: equivalent moles of CO2 = 1.6364 x 2

                                                        = 3.2727 moles

Mass of 3.2727 moles of CO2 = moles x molar mass

                                                = 3.2727 x 44.01

                                                  = 144.03 g

More on stoichiometric calculations can be found here: https://brainly.com/question/8062886?referrer=searchResults

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