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2C2H2(g)+5O2(g)=4CO2(g)+2H2O(g)

How many liters of C2H2 are required to product 12.0 moles CO2, assuming the reaction is at STP?

2C2H2g5O2g4CO2g2H2Og How Many Liters Of C2H2 Are Required To Product 120 Moles CO2 Assuming The Reaction Is At STP class=

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Eduard22sly

The volume of ethyne, C₂H₂ required to produce 12 moles of CO₂ assuming the reaction is at STP is 134.4 L

Balanced equation

2C₂H₂(g) + 5O₂(g) --> 4CO₂(g) + 2H₂O(g)

From the balanced equation above,

4 moles of CO₂ were produced by 2 moles of C₂H₂

How to determine the mole of C₂H₂ needed to produce 12 moles of CO₂

From the balanced equation above,

4 moles of CO₂ were produced by 2 moles of C₂H₂

Therefore,

12 moles of CO₂ will be produce by = (12 × 2) / 4 = 6 moles of C₂H₂

How to determine the volume (in L) of C₂H₂ needed at STP

At standard temperature and pressure (STP),

1 mole of C₂H₂ = 22.4 L

Therefore,

6 moles of C₂H₂ = 6 × 22.4

6 moles of C₂H₂ = 134.4 L

Thus, we can conclude that the volume of C₂H₂ needed for the reaction at STP is 134.4 L

Learn more about stoichiometry:

https://brainly.com/question/14735801

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