Question

Consider the following intermediate chemical equations. 2 equations. First: upper C (s) plus one half upper O subscript 2 (g) right arrow upper C upper O (g). Second: upper C upper O (g) plus one half upper O subscript 2 (g) right arrow upper C upper O subscript 2 (g). How will oxygen appear in the final chemical equation? Upper O subscript 2 (g). As a product Upper O subscript 2 (g). As a reactant O(g) as a product 2O(g) as a reactant.

Answer 1

Answer:

34.2

Explanation:

Bc it is the loser one to it

Answer 2

The oxygen in the final equation appears as reactant Upper O subscript 2 (g). Thus, option A is correct.

The chemical equations are the representation of the chemical formula involved in the equation as the reactant and the formed product.

What will be the form of oxygen?

The given chemical equations are:

1. $\rm C\;(s)\;+\;\frac{1}{2}\;O_2\;(g)\rightarrow\;CO\;(g)$
2. $\rm CO\;(g)+\;\frac{1}{2}\;O_2\;(g)\rightarrow\;CO_2\;(g)$

The final chemical equation formed for the formation of Carbon dioxide is the sum of the two equations.

The final equation is achieved by substituting equation 1 in equation 2.

$\rm C\;(s)\;+\;\frac{1}{2}\;O_2\;(g)\;+\;\dfrac{1}{2}\;O_2\;(g)\;\rightarrow\;CO_2\;(g)\\\\ C\;(s)\;+\;O_2\;(g)\;\rightarrow\;CO_2\;(g)$

The oxygen in the final equation appears as reactant Upper O subscript 2 (g). Thus, option A is correct.

Learn more about the final equation, here:

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