A reaction has two reactants Q and P. What is the order with respect to each reactant and the overall order of the reaction described by the following rate expression?       a. rate = k1                                    b. rate = k2 [P]2 [Q]       c. rate = k3 [Q]2                           d. rate = k4 [P] [Q] What will the units of the rate constants above be if the rate is expressed in M/min?

. For the following generic reaction: a A + b B -- > c C + d DWhat is the rate of reaction (rate expression) as a function of change in concentration (e.g. Δ[A]) andchange in time (Δt)?Describing Chemical Kinetics:1. Measuring RateThe rate of a chemical reaction is determined by:A. Change of moles of reactants/products over change in timeB. Change of grams of reactants/products over change in timeC. Change in concentration over change in timeD. change in volume over change in timeWrite the rate expressions based on the definition above for:a A + b B -- > c C + d Da A -- > productsDoes the order in reactant (m, n) in the rate law have anything to do with the coefficients of the reactants?

For the following reaction  2M + N →Y + 3P  identify the correct general rate law.  a.  rate = [M]2[N][Y][P]3    b.   rate = [M]m[N]n    c.  rate = k[M]m[N]n  d.   rate = k[2M]m[N]n[Y]y[3P]p     e. rate = k[2M]m[N]

The data for the reaction given NOCI (g) The following experimental data was measured for the reaction. Use the Method of Initial Rates to determine the rate law equation for this reaction 1 2 3 NO (g) + 1/2 Cl2₂ (g) [NO] [Cl₂] Initial Rate Experiment (mol.L-¹) (mol.L-¹) (mol.L-¹ s¯¹) 1.4x10-6 2.8x10-6 5.6x10-6 0.250 0.250 0.500 0.250 0.500 0.250 → 1. Determine the order of the reaction with respect to NO oxide 2. Determine the order of the reaction with respect to Cl₂ 3. What is the overall order of this reaction? 5. Calculate the value of the rate constant, k → 4. Select the correct rate law (rate equation) for this reaction: Rate =

Hydrogen peroxide, H₂O₂ (aq), decomposes to H₂O₂(l) and Q₂ (g) in a reaction that is first-order in H₂O₂ and has a rate constant k = 1.06 × 10-³ min-¹ at a given temperature. a. How long will it take for 10.% of a sample of H₂O₂ to decompose? min b. How long will it take for 86% of the sample to decompose? min

The expression, rate = k[A][B]2, would suggest which of the following steps to be the rate determining step in the overall reaction?    step 1 A + B →    C  step 2 C + B →    D + E  step 3 D + A →    products  overall:           2A + 2B →    products   A. step1   B. step2   C. step3   D. overall reaction

Chem q 5

considering the balanced equation: 2 N2H4 + N2O4 --> 3N2 + 4 H2O   Write the rate law for the dependence of the rate on concentration of the reactants, leaving the experimentally determined values as symbols: rate=K [   ]n etc

1. For the reaction A -> products, successive half-lives are observed to be 8.0, 4.0, and 2.0 minutes for an experiment in which [A]0 = 0.20 M. a. write the differetial rate law for this reaction B. write the integrated rate law for the reaction