Consider the hydrolysis of t-butyliodide,(CH3)3I + H2O → (CH3)3COH + HIThe equation governing the rate of this reaction israte = k[(CH3)3I]What is the order of reaction with regard to (CH3)3I?Group of answer choices1st order0th order1/2 order2nd order

Consider the hydrolysis of t-butyliodide,(CH3)3I + H2O → (CH3)3COH + HIThe equation governing the rate of this reaction israte = k[(CH3)3I]What will happen to the initial rate if the concentration of (CH3)3I is doubled?Group of answer choicesit will be quadrupledit will be doubledit will remain unchanged

For the following reaction…BrO3–  +  5Br–  +  6H+  →  3 Br2  +  3H2OThe rate law is…Rate = k[BrO3–][Br–][H+]2What is the order of reaction with respect to H+?Group of answer choices3rd order0th order2nd order1st order

If the rates of reaction are R1 and R2 at concentrations C1 and C2 of a reactant respectively, the order of reaction n (assuming that the concentrations of all other reactants and T remains constant) with respect to that of reactant is given by

Calculate the overall order of the reaction whose rate law expression was predicted as :Rate =k[NO]3/2 [O ]1/2

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. *