Question

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?
mol CO2

Answer 1

70 mol

the next one is 67.2

Step-by-step explanation:

:) have a great day

Answer 2

70mol

Step-by-step explanation:

The equation of the reaction is given as:

2C₂H₂ + 5O₂ → 4CO₂ + 2H₂O

Given parameters:

Number of moles of acetylene = 35.0mol

Number of moles of oxygen in the tank = 84.0mol

Unknown:

Number of moles of CO₂ produced = 35.0mol

Solution:

From the information given about the reaction, we know that the reactant that limits this combustion process is acetylene. Oxygen is given in excess and we don't know the number of moles of this gas that was used up. We know for sure that all the moles of acetylene provided was used to furnish the burning procedure.

To determine the number of moles of CO₂ produced, we use the stoichiometric relationship between the known acetylene and the CO₂ produced from the balanced chemical equation:

From the equation:

2 moles of acetylene produced 4 moles of CO₂

∴ 35.0 mol of acetylene would produced:

`(35 x 4)/(2)` = 70mol