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Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined Very often, 3 reaction does not tell us the whole story. For instance, the reaction NO2(g) + CO(g)+NO(g) + CO2(9) does not involve a collision between an NOz molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: 1. NO2(g) + NO2(a)+NOs(g) + NO(a) 2. NOs(9) + CO(g)+CO2(g) + NO2(q) Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism Overall, the resulting reaction is NO2(g) + CO(g)+NO(g) + CO2(g) Notice that in the elementary steps NOs appears both as a product and then as a reactant; therefore it cancels out of the final chemical equation. NOs is called 3 reaction intermeaiate. Also notice that 2 molecules of NQ3 appear in the reactants of the first step and 1 molecule of NO appears as product of the second step, the net effect leaves only 1 molecule of NQz as a reactant in the net equation. Molecularity is the proper term for "how the molecules collide" in a reaction. For example. step 1 is bimolecular because it involves the collision of two molecules. Step 2 is also bimolecular for the same reason. Unimolecular reactions involve only one molecule in the reactants. Though rare, collisions among three molecules can occur. 'Such a reaction would be called termolecular. Which species is a reaction intermediate? View Available Hint(s) ~ Correct Part C What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C) type k*[A]*[c]*3. View Available Hint(s) Rate = Part D What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C[ type k*[A]*[c]*3. View Av: ble Hint(s) Rate =