Carbon monoxide and oxygen react to form carbon dioxide according to the following balanced chemical equation

2 CO(g) + O2(g) ➔ 2 CO2(g)

If CO(g) and O2(g) are combined in the ratio shown in the diagram below, where the black spheres represent carbon atoms and the red spheres represent oxygen atoms, which molecules will remain when the reaction is complete?

Question

Carbon monoxide and oxygen react to form carbon dioxide according to the following balanced chemical equation

2 CO(g) + O2(g) ➔ 2 CO2(g)

If CO(g) and O2(g) are combined in the ratio shown in the diagram below, where the black spheres represent carbon atoms and the red spheres represent oxygen atoms, which molecules will remain when the reaction is complete?

BlackTom AI · Accepted Answer

The question presents the balanced chemical equation: 2 CO(g) + O2(g) → 2 CO2(g). The scenario asks which molecules will remain once the reaction has gone to completion given the ratio of reactants shown in the diagram.

Option 1: 'CO2 and O2 molecules' — This would imply that all CO has been consumed while some O2 remains unreacted, producing CO2 from the CO that did react. However, the reaction uses CO and O2 in a 2:1 ratio to make CO2; if O2 were in excess, you would expect CO to be exhausted first, leaving CO2 and leftover O2, not CO2 and O2 alone. The combination described does not fit a straightforward stoichiometric outcome where O2 remains without any CO or CO2 after all CO is consumed.

Option 2: 'Only CO2 molecules' — This would occur if both CO and O2 were completely consumed with no excess reactants left. That situation happens only if the initial amounts of CO and O2 are exactly in the stoichiometric proportions to form CO2 with no leftovers. If the diagram shows an excess of one reactant (which is typical in such problems to create leftover species), this option would be incorrect. Additionally, even with CO2 formed, if one reactant is in excess, some of it would remain unreacted, so you would not end up with only CO2 molecules.

Option 3: 'CO2 and CO molecules' — This outcome corresponds to a scenario in which all O2 is consumed (limiting reagent) and an excess of CO remains. The reaction would convert the available O2 and twice as much CO into CO2, leaving some CO unreacted. Thus, the mixture after reaction would consist of CO2 (the product) and leftover CO molecules (unreacted starting material). This option aligns with a common stoichiometric outcome when O2 is limiting relative to CO.

Option 4: 'CO and O2 molecules' — If this were the final state, it would imply no reaction occurred and all reactants remained as their original diatomic/monatomic forms. That contradicts the given balanced equation, which shows CO and O2 do react to form CO2. Therefore, this scenario cannot be correct for a completed reaction under the given conditions.

Option 5: 'I am unsure and need to study this concept to prepare for the exam' — While asking for study is perfectly reasonable in learning contexts, this choice does not engage with the chemical reasoning required by the problem. It would not be the appropriate selection for a question that can be answered through stoichiometric analysis.

In summary, the correct reasoning involves comparing the stoichiometric needs (2 CO per 1 O2 to produce 2 CO2) to the actual quantities shown in the diagram. If the diagram indicates that O2 is the limiting reagent, then all O2 will be consumed and CO will be left over, resulting in a mixture of CO2 and CO after the reaction completes. Conversely, if CO were limiting, you’d expect CO2 and O2 remaining, not CO2 and CO. The other options fail to align with these stoichiometric consequences or imply no reaction occurs, which contradicts the given equation.

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