25. For the reaction, 2H₂S(g) + O₂(g) → 2S(s) + 2H₂O(), which one of the following statements is absolutely true? (a) The reaction is first order with respect to H₂S and second order with respect to 02. (b) The reaction is fourth order overall. (c) The rate law is: rate = K[H₂S]²[0₂]. (d) The rate law is: rate = k[H₂S][0₂]. (e) The rate law cannot be determined from the information given.

Assume that the formation of nitrogen dioxide: 2NO(g) + O2(g) 2NO2(g)   is an elementary reaction. (a) Write the rate law for this reaction. (b) A sample of air at a certain temperature is contaminated with 2.0 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. (c) Under the conditions described in part (b), the half-life of the reaction has been estimated to be 6.4 × 103 min. What would the half-life be if the initial concentration of NO were 10 ppm?

1. Given the following mechanism for the catalytic destruction of ozone: O3 Оз 02 + 0 O3 + 0 202 (a) Write the overall reaction. (b) What is the intermediate? Explain why. (c) Write all the rate laws for each step (in terms of [O3]). (d) The rate determining step is given as the step 2. Use the steady state approximation to derive the rate law.

For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (For each answer, enter an exact number as an integer or decimal.) (a) rate = k [X]° [Y]° Z] X Y Overall (b) rate = k [X]/?[Y]³3/² [Z]-1 X Y Z Overall rate = k [z]? (c) X Y Overall

Which of the following statements about rate laws is FALSE? A) Rate laws can only be determined experimentally. B) Rate laws tell us information about the mechanism of the chemical reaction under study. C) The rate law for the chemical reaction A + B + 20 –D must be rate = k[A][B][C]² %3D D)A rate law can only be written for the elementary reactions of a given chemical reaction.

Consider the following reaction: 2A + B + 3C. (a) Write an expression for the overall rate; (b) What are the rates at which A and B are consumed and generated if C is created at a rate of 0.015 M/min?

5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T

Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO₂(g)] [03(g)] Rate = k [NO₂(g)]² [03(g)] Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(g)] (b) If the rate constant for this reaction at a certain temperature is 97900, what is the reaction rate when [NO₂(g)] = 0.587 M and [03(9)] = 1.40 M? Rate = 2 NO₂(g) + 03(9) → N₂O5(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.17 M while the concentration of O3(g) is 1.40 M? M/S

The rate law for the reaction NO2(g) + O2(g) is given by rate = - k[NO₂] NO(g) + 03 (g) If the following is the mechanism for the reaction, which of the following statements correctly describe the reaction? Check all that apply. NO2(g) NO(g) + O(g) - O(g) + O2(g) 03 (g) The reaction is 2nd order overall. The first step is the slow step. Doubling NO, would quadruple the rate. Cutting O, in half would decrease the rate by a factor of 2. The molecularity of the first step is 1. Both steps are termolecular. None of the above

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: (b) For a reaction of the form, A + B + C --> reaction from the choices below. (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A] [B]Y? Choose all correct possibilities. O [A] = 0.2 and [B] = 1.0 O [A] = 0.4 and [B] = 1.0 O [A] = 0.8 and [B] = 0.5 O [A] = 0.6 and [B] = 0.5 O [A] = 0.2 and [B] = 1.5 O [A] = 0.4 and [B] = 0.5 O [A] = 0.4 and [B] = 1.5 O [A] = 1.0 and [B] = 0.5 O Rate = K[A][B][C] O Rate = K[A][C] O Rate = K[A]²[C] T O Rate = k[A][C]² O Rate = K[A]²[C]² O Rate = K[A]³ [c] O Rate = K[A][C]³ the following Experiment [A] (M) [B] (M) Rate (M/s) 0.5 0.5 The rate will be the original rate multiplied by a factor of 0.2 0.4 (c) By what factor will the rate of the reaction described in part (b) above change if the…