The balanced equation for combustion in an acetylene torch is shown below:
2C2H2 + 5O2 → 4CO2 + 2H2O

The acetylene tank contains 35.0 mol C2H2, and the oxygen tank contains 84.0 mol O2.

How many moles of CO2 are produced when 35.0 mol C2H2 react completely?
and

How many moles of CO2 are produced when 84.0 mol O2 completely react?

The answer to your question is a) 70 moles of CO₂

                                                     b) 67.2 moles of CO₂

Explanation:

Data

moles of C₂H₂ = 35

moles of O₂ = 84

Balanced chemical equation

                 2C₂H₂  +  5O₂   ⇒   4CO₂  +  2H₂O

Process

1.- Moles of CO₂

                2 moles of C₂H₂ 4 moles of CO₂

              35 moles of C₂H₂  x

                                         x = (35 x 4)/2

                                        x = 70 moles of CO₂

2.- Moles of CO₂

                5 moles of O₂ 4 moles of CO₂

               84 moles of O₂  x

                                  x = (84 x 4) / 5

                                  x = 67.2 moles of CO₂

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