For the elementary reaction
NO 3 + CO → NO2 + CO 2
the molecularity of the reaction is __________, and the rate law is rate = __________.
A) 2, k[NO 2][CO 2]
B) 2, k[NO 3][CO]/[NO2 ][CO 2]
C) 4, k[NO 3][CO][NO 2][CO 2]
D) 4, k[NO 2][CO 2]/[NO 3][CO]
E) 2, k[NO 3][CO]
how do i solve problems like these?
I think the secret is the wording. In "elementary" reactions, you go with the coefficients in the balanced equation.
So reactions involving 1 molecule are unimolecular, while two or three or either bimolecular or termolecular. So this is a bimolecular equation and the rate law is k[NO3][CO] so I would go with answer E.
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To determine the molecularity of a reaction, you need to count the number of reactant particles or species involved in the elementary reaction. In this case, the reaction has two reactant species: NO3 and CO. Therefore, the molecularity of the reaction is 2.
To determine the rate law of the reaction, you need experimental data or information about the reaction mechanism. However, from the given options, you can see that the rate law contains different concentrations of the reactants and/or products raised to various exponents, along with the rate constant (k).
To deduce the correct rate law, you should consider the stoichiometry of the balanced equation. In this case, the stoichiometric coefficient of NO3 is 1, while the coefficient of CO is also 1. Therefore, the rate law should include [NO3] and [CO] as reactant concentrations.
Looking at the options, we can see option E) 2, k[NO3][CO] matches this requirement. Hence, the correct answer is E) 2, k[NO3][CO].
To solve problems like these, you need to carefully analyze the given balanced equation, identify the number of reactant particles (molecularity), and consider the stoichiometry to determine the rate law. If experimental data or information about the reaction mechanism is provided, you can use that to confirm the rate law.