What is the rate law for N2O4+CO yields NO+CO2+NO2?
To determine the rate law for a given reaction, you need experimental data that includes the initial concentrations of the reactants and the observed reaction rates at those concentrations.
In this example, the reaction being considered is N2O4 + CO → NO + CO2 + NO2.
To experimentally determine the rate law, you can carry out multiple experiments varying the initial concentrations of the reactants and measuring the corresponding rates. By comparing the rates obtained in different experiments, you can determine the effect of changing the concentrations of the reactants on the rate of the reaction.
Assuming the rate law follows the general form rate = k[A]^m[B]^n, where [A] and [B] represent the concentrations of the reactants, and k is the rate constant, you would need to determine the values of m and n, as well as the rate constant k.
Here's how you can experimentally determine the rate law:
1. Choose a specific initial concentration for one of the reactants (let's say [A]) and keep the concentration of the other reactant ([B]) constant.
2. Measure the initial rate of the reaction under these conditions.
3. Repeat the experiment, but this time modify the concentration of [A] while keeping [B] constant. Measure the rate again.
4. If changing the concentration of [A] while keeping [B] constant affects the rate, then the rate law must include [A] as a term. If changing [B] affects the rate, then the rate law must include [B] as a term.
5. By comparing the two experiments, you can determine the values of m and n in the rate law equation.
6. Repeat this process for different concentrations and combinations of reactants to confirm the rate law.
Once the rate law is determined, it can be used to predict the rate of the reaction at any given set of reactant concentrations.
It's important to note that the rate law can only be determined experimentally and may not always match the stoichiometric coefficients of the reaction.