Question

Consider the following intermediate chemical equations. C(5)+ 0₂(g) → CO(g) CO(g)+ 0₂(g) - C02(0) How will oxygen appear in the final chemical equation? O₂(g) as a product O₂(g) as a reactant OO(g) as a product 20(g) as a reactant

a) O₂(g) as a product
b) O₂(g) as a reactant
c) OO(g) as a product
d) 2O(g) as a reactant

Answer 1

In the final chemical equation after combining the provided intermediate equations, oxygen (O₂(g)) appears as a reactant, not a product. The correct answer is b) O₂(g) as a reactant.

Step-by-step explanation:

When analyzing the intermediate chemical equations and combining them, oxygen (O₂(g)) will appear as a reactant in the final chemical equation, not as a product. The correct combination of the provided equations would yield 2 C(s) + O₂(g) → 2 CO(g), then CO(g) + ½O₂(g) → CO₂(g). The overall balanced reaction when these are combined and simplified is C(s) + O₂(g) → CO₂(g), where oxygen gas is consumed in the reaction as a reactant to produce carbon dioxide.

The presence of different possible orientations for collisions, such as when CO(g) and O₂(g) collide to form CO₂(g), highlights the importance of molecular orientation in the reaction. However, the presence of such collision orientations does not change the role of O₂(g) as a reactant in the overall equation.

Therefore, the correct answer to how oxygen will appear in the final chemical equation is as a reactant, which corresponds to option b) O₂(g) as a reactant.