(a) H₂O₂ → H₂O + O (b) Br+ Br + M (c) NO₂ + NO₂ Br₂ + M 2 NO + 0₂ unimolecular bimolecular termolecular ŷ rate = rate = rate =

Using the information in the table, the value of the rate constant TOP A(g) + B(g) → C(g) + D(g) is [A], (M) 0.100 0.200 0.300 [B], (M) 2.50 Jay 2.50 1.25 Rate (M/s) 0.460 0.920 1.38 A) 4.6 s¹ B) 0.046 s¹ C) 1.84 M¹s¹ D) 115 M²S-1 E) 0.42 s¹

Consider a reaction A + B → C with corresponding rate law rate = k[A]n [B]m If n = 2, m = 1: (d) How will the initial reaction rate change if the initial concentration of A is doubled, without changing the initial concentration of B? (e) How will the initial reaction rate change if the initial concentrations of both A and B are doubled?

The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?

Consider the following Potential Energy Diagram for a four-step reaction mechanism.  (a)              What is the overall balanced equation for the reaction? (b)              Does this reaction have a catalyst? Explain how you know.   (c)          Which step in the above mechanism is the rate-determining step? (d)          Is this reaction exothermic or endothermic?   (e)      The rate law equation was determined to be rate = k [NO2] [F2].  Is the proposed mechanism           plausible?

Consider the reaction 2NO(g) + O2(g) → 2NO2(g) Suppose that at a particular moment during the reaction nitric oxide (NO) is reacting at the rate of 0.066 M/s. (a) At what rate is NO2 being formed? (b) At what rate is molecular oxygen reacting?

(a) Consider the chlorination of methane, given below: 1 CH4(g) + 4 Cl2(g)  1 CCl4(g) + 4 HCl(g) If CH4(g) is decreasing at the rate of 0.600 mol/s, what are the rates of change of Cl2(g), CCl4(g), and HCl(g)?Cl2(g)/t =  CCl4(g)/t =  HCl(g)/t =  (b) The decomposition reaction given below: 2 N2O5(g)  4 NO2(g) + 1 O2(g) is carried out in a closed reaction vessel. If the partial pressure of N2O5(g) is decreasing at the rate of 806 torr/min, what is the rate of change of the total pressure in the vessel?Ptot /t =

ki [2] Given the mechanism: NO(g) + O2(g) SNO;(g) [fast, reversible] k-1 (1) k2 NO:(g) + NO(g) → 2NO2(g) [slow] (2) (a) Write the equation for the overall reaction. (b) Which step is rate determining? (c) Which species is an intermediate? (d) Which species is a catalyst? (e) What is the rate law predicted by the above mechanism for the overall reaction?

The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [O₂(g)]² [NO(g)]²2 O Rate = k [O₂(g)] [NO(g)]³ O Rate = k [0₂(g)]4 [NO(g)] (b) What is the value of the rate constant? Experiment M/s 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?

Identify each of the following elementary reactions as uni- molecular, bimolecular, or termolecular, and write the rate expression. (a) HCO + O2 → HO2 + CO (b) CH3 + O2 + N2 → CH;O2 + N2 (c) HO,NO2 –→ HO2 + NO2