When the rate of the reversible reaction A + BSC is studied under a certain set of conditions, it is found that the rate of the forward reaction is kA]. What can be concluded about the rate law for the reverse reaction under these conditions? (A) Rate = k-[C] %3D (B) Rate = k [B] (C) The rate law of the reverse reaction cannot be determined from the information given. (D) An crror must have been made, since if the reaction is reversible, the forward rate law must be Rate = k{A][B]. %3D

In a study of the formation of HI from its elements, H2(g) + 12(g) == 2HI(g) equal amounts of H2 and 12 were placed in a container, which was then sealed and heated. (a) On one set of axes, sketch concentration vs. time curves for H and HI, and explain how Q changes as a function of time. (b) Is the value of Q different if [12] is plotted instead of [H2]?

For the reaction of the ammonium ion with nitrous acid, the net reaction is NH4*(aq) + HNO2(aq) → N2(g) + 2H2O() + H*(aq) If the initial concentration of nitrous acid is 1.00 M and, after 28.8 s has elapsed, the concentration of nitrous acid has fallen to 0.82 M, what is the average rate of the reaction over this time interval? 0.0063 M/s 0.028 M/s -0.0063 M/s -0.028 M/s O 0.063 M/s

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The activation energy for the isomerization reaction CH3NC(g) → CH3CN(g) is 161 kJ mol−¹, and the reaction rate constant at 600 K is 0.41 s¯¹. (a) What is the value of the pre-exponential factor A for this reaction? (b) What is the value of the rate constant of the reaction at 1000 K?

The rate constant of the elementary reaction BH, (aq) + NH (aq) → BH;NH3 (aq) + H2 (g) is k = 1.94 x 10-4L mol¯' s-' at 30.0°C, and the reaction has an activation energy of 161 kJ mol. (a) Compute the rate constant of the reaction at a tem- perature of 40.0°C. (b) After equal concentrations of BH (aq) and NH, (aq) are mixed at 30.0°C, 1.00 × 10ª s is required for half of them to be consumed. How long will it take to consume half of the reactants if an identical experi- ment is performed at 40.0°C?

Certain bacteria use the enzyme penicillinase to decom- pose penicillin and render it inactive. The Michaelis- Menten constants for this enzyme and substrate are Km = 5 × 10-5 mol L-ªand k, = 2 × 10³ s¯1. (a) What is the maximum rate of decomposition of peni- cillin if the enzyme concentration is 6 × 10-7 M? (b) At what substrate concentration will the rate of decomposition be half that calculated in part (a)?

Show below in the table are the data from the decomposition of N2O5 in CCl4 at 45°C: Initial concentration Initial rate, Ms-1 of [N2O5], M 0.50 -4 1.55 × 10 3.10 × 10-4 4.65 × 104 (a) Determine the order of the reaction (decomposition process). 1.0 1.5 (b) Calculate the value of k. (c) Then calculate the half-life of the above decomposition reaction.

7.) The results of kinetics experiments have shown the rate of the following reaction:A + 2B + C ↓ products has the following rate law: rate = k[A]2[B]0[C]1with a rate constant of k = 1.3 × 10–4 L2/mole2·s (M –2·s–1).a.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 0.3, and 0.4 M, respectively?b.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 2.7, and 0.4 M, respectively?

5. The collision theory of reaction rates states that the rate of a reaction depends on the number of collisions between mol- ecules, the average energy of the collisions, and the effectiveness of the collisions. (a) How does temperature affect each of these factors in collision theory? (b) Does the effect of temperature on the reaction rate support the collision theory of reaction rates? Explain.