Below are the elementary steps that make-up the reaction mechanism for the following reaction.F2 + 2 NO2 → 2 NO2FStep 1: F2 + 2 NO2 → NO2F + F + NO2 (slow)Step 2: F + NO2 → NO2F (very fast)Which is the rate determining step?Group of answer choicesStep 1Step 2

A level chemistry ocr a question) Which statement about the rate-determining step of a reaction is correct: A- It is the fast step, B- It cannot involve a catalyst, C- it doesn't involve 0 order reagents, D- it is always between two first order reagents

NO 2 reacts with Cl2 gas to form NO 2 Cl:2 NO 2 (g) + Cl2 (g) ® 2 NO 2 Cl (g)The following mechanism has been proposed:NO 2 (g) + Cl2 (g) ® NO 2 Cl (g) + Cl (g) (slow)NO 2 (g) + Cl (g) ® NO 2 Cl (g) (fast)Determine the rate law for the reaction

Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism:step elementary reaction rate constant1 NO2(g) → NO(g) + O(g) k12 O(g) + NO2(g) → O2(g) + NO(g) k2Suppose also k1≪k2. That is, the first step is much slower than the second.Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. =k

define ‘chemical kinetics’; *9.2 Rate and Order of Reaction 9.2.1 define the terms:a. rate of reactionb. rate lawc. order of reactiond. rate constante. rate determining step;*9.2.2 explain the significance of the rate determining step on theoverall rate of a multistep reaction;*9.2.3 determine the rate law for the given reactions; *9.2.4 deduce the order of reaction using the method of initial rate; *9.3 Collision Theory, Transition Stateand Activation Energy9.3.1 relate activation energy and activated complex to the rate ofreaction;*9.3.2 calculate the initial rate using concentration data of givenreactions;*9.3.3 draw a labelled energy diagram for a chemical reactionrepresenting the activation energy and the effect of catalyst;*9.3.4 describe collision theory; *9.3.5 explain the effect of concentration, temperature and surfacearea on rate of reaction by using collision theory;*9.4 Catalysis 9.4.1 define the term ‘catalyst’; *9.4.2 explain homogeneous and heterogeneous catalysis; *9.4.3 explain the effect of catalyst on the rate of reaction. *

Study the following reaction energy diagram:0reactantsenergyproductsThen answer the following questions about the chemical reaction.Does this reaction release or absorb energy? releaseabsorbneitherHow many transition states occur duringthis reaction? Could this be an elementary reaction? yesnoIf you said this reaction could not be elementary, then how many steps are in its mechanism? If you said this reaction could not be elementary, then enter the number of the step in its mechanism which is rate-determining. For example, if the first step is the rate-determining step, enter "1" here.