consider the following intermediate chemical equations.\n c(s)+\frac{1}{2}o_2(g)\rightarrow co(g) \n…

consider the following intermediate chemical equations.\n c(s)+\frac{1}{2}o_2(g)\rightarrow co(g) \n co(g)+\frac{1}{2}o_2(g)\rightarrow co_2(g) \nwhen you form the final chemical equation, what should you do with co?\ncancel out co because it appears as a reactant in one intermediate reaction and a product in the other intermediate reaction.\nadd the two co molecules together, and write them as reactants in the final chemical reaction.\nwrite co only once as a reactant in the final chemical reaction.\nwrite co as a reactant and a product in the final chemical reaction.

consider the following intermediate chemical equations.\n c(s)+\frac{1}{2}o_2(g)\rightarrow co(g) \n co(g)+\frac{1}{2}o_2(g)\rightarrow co_2(g) \nwhen you form the final chemical equation, what should you do with co?\ncancel out co because it appears as a reactant in one intermediate reaction and a product in the other intermediate reaction.\nadd the two co molecules together, and write them as reactants in the final chemical reaction.\nwrite co only once as a reactant in the final chemical reaction.\nwrite co as a reactant and a product in the final chemical reaction.

Answer

Brief Explanations:

In chemical equation - addition, a species that appears as a product in one step and a reactant in another is an intermediate. Intermediates are canceled out when forming the overall reaction. Here, CO is a product in the first reaction and a reactant in the second reaction.

Answer:

Cancel out CO because it appears as a reactant in one intermediate reaction and a product in the other intermediate reaction.