Nitrogen dioxide (NO2) reacts with ozone (O3) according to the equation: 2NO2(g)
ID: 998582 • Letter: N
Question
Nitrogen dioxide (NO2) reacts with ozone (O3) according to the equation:2NO2(g) + O3(g) ------> N2O5(g) + O2(g)
If the rate law for this reaction is rate=k[NO2][O3], what is the overall order of the reaction? Nitrogen dioxide (NO2) reacts with ozone (O3) according to the equation:
2NO2(g) + O3(g) ------> N2O5(g) + O2(g)
If the rate law for this reaction is rate=k[NO2][O3], what is the overall order of the reaction?
2NO2(g) + O3(g) ------> N2O5(g) + O2(g)
If the rate law for this reaction is rate=k[NO2][O3], what is the overall order of the reaction?
Explanation / Answer
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In chemical kinetics, the rate of a reaction is proportional to the concentration of reactants. The proportionality constant k is called the rate constant. The rate law expresses the relationship of the rate of a reaction to the rate constant and the concentrations of the reactants. This concentrations are, in general, raised to some power. For the reaction that you have the general rate law would be: rate = k[NO2]x[O3]y, where x and y are numbers that must be determined experimentally. In this case, since you are given the rate law, x=y=1. Notice that x and y are not necessarily equal to the stoichiometric coefficients 2 and 1.
Exponents x and y specify the relationships between the concentration of reactants, in this case NO2 and O3, and the reaction rate. Added together, they give us the overall reaction order. The reaction order is defined as the sum of the powers to which all reactant concentrations that appear in the rate law are raised. For this reaction, given the data we have the overall order of the reaction will be two (2).
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