Fwdaf

Ch. 14 Practice Problems: Chemical Kinetics (Show all work on a separate sheet of paper in a neat, organized fashion) 1. Write the rate expressions for the following reactions in terms of the disappearance of the reactants and the appearance of the products: (**note** do not include pure solids or pure liquids in the rate expressions!!!) a. I-1(aq) + OCl-1(aq) ( Cl-1(aq) + OI-1(aq) b. 4NH3(g) + 5O2(g) (4NO(g) + 6H2O(g) c. H2(g) + I2(g) ( 2HI(g) d. 5 Br-1(aq) + BrO3-1(aq) + 6H+1(aq)(3Br2(aq) + 3H2O(ℓ) e. 2H2(g) + O2(g) ( 2H2O(g) 2. Consider the reaction: 2NO(g) + O2(g) ( 2NO2(g) Suppose that at a particular moment during the reaction nitrogen monoxide 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' 3. a. The rate law for the reaction: NH4+1(aq) + NO2-1(aq) ( N2(g) + 2H2O(ℓ) is experimentally determined to be Rate=k [NH4+1]1[NO2-1]1. At 25oC, the rate constant is 3.0x10-4 M-1•s-1. Calculate the rate of the reaction at this temperature if [NH4+1] =0.26M and [NO2-1] =0.080M. b. The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5(4NO2 + O2. The rate law is first order in N2O5. At 64oC the rate constant is 4.82x10-3 s-1. (a) Write the rate law for the reaction. (b)What is the rate of the reaction when [N2O5] =0.0240M' (c)What happens to the rate when the concentration of N2O5 is doubled to 0.0480 M' 4. Given the data in the table below, use the method of initial rates to determine the Rate Law, the overall order of the reaction, and the value of the rate constant, k, (using exp #1) for the reaction: F2 (g) + ClO2 (g) ( 2FClO2 (g) | |[F2] (M) |[ClO2] (M) |Initial Rate (M/s) | |Exp#1 |0.10 |0.010 |1.2x10-3 | |Exp#2 |0.10 |0.040 |4.8x10-3 | |Exp#3 |0.20 |0.010 |2.4x10-3 | 5. Given the data in the table below, use the method of initial rates to determine the Rate Law, the overall order of the reaction, and the value of the rate constant, k, (using exp #1) for the reaction: 2NO (g) + 2H2 (g) ( N2 (g) + 2H2O (g) | |[NO] (M) |[H2] (M) |Initial Rate (M/s) | |Exp#1 |5.0x10-3 |2.0x10-3 |1.3x10-5 | |Exp#2 |10.0x10-3 |2.0x10-3 |5.0x10-5 | |Exp#3 |10.0x10-3 |4.0x10-3 |10.0x10-5 | 6. Given the data in the table below, use the method of initial rates to determine the Rate Law, the overall order of the reaction, and the value of the rate constant, k, (using exp #1) for the reaction: S2O8-2(aq) + 3I-1(aq) ( 2SO4-2(aq) + I3-1(aq) | |[S2O8-2] (M) |[I-1] (M) |Initial Rate (M/s) | |Exp#1 |0.080 |0.034 |2.2x10-4 | |Exp#2 |0.080 |0.017 |1.1x10-4 | |Exp#3 |0.16 |0.017 |2.2x10-4 | 7. Given the data in the table below, use the method of initial rates to determine the Rate Law, the overall order of the reaction, and the value of the rate constant, k, (using exp #1) for the reaction: CH3COCH3 + Br2 + H+1 ( CH3COCH2Br + H+1 + Br-1(aq) | |[CH3COCH3] (M) |[Br2] (M) |[H+1] (M) |Initial Rate (M/s) | |Exp#1 |1.00 |1.00 |1.00 |4.0x10-3 | |Exp#2 |2.00 |1.00 |1.00 |8.0x10-3 | |Exp#3 |2.00 |2.00 |1.00 |1.6 x10-2 | |Exp#4 |1.00 |2.00 |2.00 |8.0x10-3 | 8. Given the data in the table below, use the method of initial rates to determine the Rate Law, the overall order of the reaction, and the value of the rate constant, k, (using exp #1) for the reaction: 2NO (g) + 2H2 (g) ( N2 (g) + 2H2O (g) | |[NO] (M) |[H2] (M) |Initial Rate (M/s) | |Exp#1 |0.10 |0.20 |0.0150 | |Exp#2 |0.10 |0.30 |0.0225 | |Exp#3 |0.20 |0.20 |0.0600 | 9. Given the data in the table below, use the method of initial rates to determine the Rate Law, the overall order of the reaction, and the value of the rate constant, k, (using exp #1) for the reaction: 2A + B ( 2C | |[A] (M) |[B] (M) |Initial Rate (M/s) | |Exp#1 |0.10 |0.20 |300. | |Exp#2 |0.30 |0.40 |3600. | |Exp#3 |0.30 |0.80 |14,400 | 10. Given the data in the table below, use the method of initial rates to determine the Rate Law, the overall order of the reaction, and the value of the rate constant, k, (using exp #1) for the reaction: A + B + C ( Products | |[A] (M) |[B] (M) |[C] (M) |Initial Rate (M/s) | |Exp#1 |0.1 |0.2 |0.3 |0.063 | |Exp#2 |0.3 |0.4 |0.2 |0.084 | |Exp#3 |0.6 |0.4 |0.2 |0.168 | |Exp#4 |0.3 |0.4 |0.1 |0.021 | |Exp#5 |0.6 |0.2 |0.2 |0.168 |