In a study of the decomposition of ammonia on a tungsten surface at 1100 °C NH31/2 N2 + 3/2 H2 the following data were obtained: NH3), M 1.17x102 5.85x10-3 441 2.93×10-3 1.47x10-3 seconds 661 771 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.17×10² M is | s and when the starting concentration is 5.85×10³ M is (2) The average rate of disappearance of NH3 from t = 0 s to t = 441 s is ]Ms'. (3) The average rate of disappearance of NH3 from t = 441 s to t= 661 s is ]Ms'. (4) Based on these data, the rate constant for this v order reaction is Ms!

In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H,(g) + % »(9) the following data were obtained: HI], M seconds 0.274 0.137 6.85×10-2 3.43x10-2 521 782 912 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.274 M is s and when the starting concentration is 0.137 M is (2) The average rate of disappearance of HI from t= 0s to t= 521 s is| Ms!. (3) The average rate of disappearance of HI from t= 521 s to t= 782 s is| Ms! (4) Based on these data, the rate constant for this | | order reaction is Ms!.

The following data are for the gas phase decomposition of sulfuryl chloride at 600 K.SO2Cl2(g) SO2(g) + Cl2(g) [ SO2Cl2 ], M 3.73×10-3 1.87×10-3 9.35×10-4 4.68×10-4   time, min 0 203 406 609 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is ________ min .(2) Based on these data, the rate constant for this _______(zero, first, or second) order reaction is __________min-1.

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The activation energy of an uncatalyzed reaction is 86 kJ/mol. The addition of a catalyst lowers the activation energy to 61 kJ/mol Part A Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 24 °C? Express the ratio to two significant digits. ke/ku = 2.2 • 1o Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Part B Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 128 °C? Express the ratio to two significant digits. ? ke/k, = 2.9 • 10² Submit Previous Answers Request Answer X Incorrect; Try Again; 8 attempts remaining

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At a certain temperature the rate of this reaction is first order in N₂O5 with a rate constant of 0.0125 s¯¹: 2N₂O5 (g) → 2N₂O4 (8) + 0₂ (8) Suppose a vessel contains N₂O5 at a concentration of 1.14M. Calculate the concentration of N₂O5 in the vessel 88.0 seconds later. You may assume no of reaction is important. Round your answer to 2 significant digits.

The hydroxyl radical in the atmosphere is most effectively removed by hydrocarbons such as methane according to the second-order reaction below. •OH + CH4 - H20 + CH3: Given that the second-order rate constant is 3.0x106 L·mol-1.s-1, calculate the lifetime of the radical at 19°C if the concentration of CH4 is 1.5×103 ppb by volume. (Hint: The lifetime of the radical is given by 1/k[CH4].) 4.0 3.55e-3

In a study of the decomposition of nitrous oxide at 565 °C N2₂O(g) N₂(g) + ½ O₂(g) the following data were obtained: [N₂0], M seconds 0.750 0 0.375 1.50x10³ 0.188 4.47x10³ Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.750 M is concentration is 0.375 M is S. (2) The average A(1/[N₂0])/ At from t = 0 s to t = 1.50x10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47x103 s is (3) Based on these data, the rate constant for this 9.40×10-2 1.04x104 M-1 S-1. order reaction is M-1 S-1. M-¹ S-1. s and when the starting

A student obtained the following data for the gas phase decomposition of phosphine at 120 °C. PH3(g) 1/4 P4(g) + 3/2 H₂(g) 9.40x10-2 [PH3], M time, s 0 4.70x10-2 29.9 2.35x10-2 1.18x10-2 89.7 59.8 (1) What is the half-life for the reaction starting at t = 0 s? What is the half-life for the reaction starting at t = 29.9 s? Does the half-life increase, decrease or remain constant as the reaction proceeds? (2) Is the reaction zero, first, or second order? (3) Based on these data, what is the rate constant for the reaction?