Final answer:
The possible reaction according to Dalton's atomic theory is N2(g) + O2(g) = 2NO(g). NO is not a catalyst in the decomposition of NO2. Adding more catalyst to a reaction at equilibrium increases the rate of achieving equilibrium without changing the concentrations of the reactants and products.
Step-by-step explanation:
The student's question pertains to reactions that are possible according to Dalton's atomic theory. Among the given options, (b) N2(g) + O2(g) = 2NO(g) is the correct answer. This reaction involves the combination of nitrogen and oxygen gases to form nitrogen monoxide (NO). According to Dalton's atomic theory, atoms can combine in simple whole number ratios to form compounds, and that is exactly what is observed in this reaction where one molecule of nitrogen reacts with one molecule of oxygen to form two molecules of nitrogen monoxide.
As for the decomposition of NO2, NO is not a catalyst since it does not remain unchanged in the reaction. Instead, it participates actively in the overall reaction. Lastly, when more catalyst is added to a reaction at equilibrium, it typically speeds up the reaction without changing the concentration of reactants and products at equilibrium. Therefore, the concentrations of H2, CO, and CH3OH would not change upon adding more catalyst but the rate at which equilibrium is achieved would increase.