If the actual yield of the reaction was 75% instead of 100%, how many molecules of O2 would be present after the reaction is over? The# of No2 molecules is 8 if it goes through completion and NO is the limiting reactant.

Question

Ace Michael

Chemistry

6 February, 20:45

If the actual yield of the reaction was 75% instead of 100%, how many molecules of O2 would be present after the reaction is over? The# of No2 molecules is 8 if it goes through completion and NO is the limiting reactant.

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Jabari Parker · Answer 1

The reaction for the production of NO₂ is as follows:

2 NO + O₂ → 2 NO₂

Then, we use stoichiometry to solve the problem. The solution is as follows:

8 molecules NO₂ (1 molecule O₂/2 molecules NO₂) (0.75) = 3

Therefore, it will need 3 molecules of oxygen for a 75% yield.