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The reaction between C₂H2O, and O₂ is represented by the balanced equation above. In an experiment, 0.30 mol of CO₂ was produced from the reaction of 0.05 mol of C₂H₂O with excess
O₂. The reaction was repeated at the same temperature and in the same container, but this time 0.60 mol of CO₂ was produced. Which of the following must be true?



Answer :

bharathparasad577

The initial amount of C2H2O  in the container must have been 0.10mol.

 C2H2O + 2 O2 = 2 CO2 + H2O

it can be clearly seen from the above reaction that 1 mol of C2H2O reacts to produce 2 mol of CO₂ and O₂ is given in excess that means the formation of product is decided by C2H2O only. So , here C2H2O is limiting reactant and O₂ is excess reactant

0.05 mol of C₂H₂O forms 0.30 mol of CO₂ which is 6 times of C₂H₂O that  has been reacted.

Now for 0.60 moles of CO₂ to form it should 0.6 divided by 6 mol of reactant that means

moles of C2H2O= 0.6/6 = 0.1 mol .


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