In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) % H2(g) + ½ I½(g) the following data were obtained: [HI], M 0.514 0.257 0.129 6.45x102 seconds 521 781 911 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.514 M is s and when the starting concentration is 0.257 M is (2) The average rate of disappearance of HI from t = 0 s to t = 521 s is ]Ms!. (3) The average rate of disappearance of HI fromt=521 s to t = 781 Common Greek(upper) Greek(lower) Arrows Other (4) X, Ox Aa (s) (1) (g) (aq) Based on these data, the rate constant for this order rea

In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) % H2(g) + ½ I½(g) the following data were obtained: [HI], M 0.514 0.257 0.129 6.45x102 seconds 521 781 911 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.514 M is s and when the starting concentration is 0.257 M is (2) The average rate of disappearance of HI from t = 0 s to t = 521 s is ]Ms!. (3) The average rate of disappearance of HI fromt=521 s to t = 781 Common Greek(upper) Greek(lower) Arrows Other (4) X, Ox Aa (s) (1) (g) (aq) Based on these data, the rate constant for this order rea

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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!.
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The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N2O5 and first order overall. The rate constant for the reaction at 70.oC is 6.82x10-3 s-1. The reaction is started with 0.300 mol of N2O5 in a 0.500L container. How many minutes will it take for the concentration of N2O5 to drop to 0.145M?
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In a study of the gas phase decomposition of nitrogen dioxide at 383 °C NO2(9)NO(g) +½ O2(g) the following data were obtained: NO2], M seconds 0.436 0.218 0.109 5.45x10-2 4.78 14.3 33.4 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.436 M is ]s and when the starting concentration is 0.218 M is (2) The average A(1/[NO2]) / At from t= 0 s to t= 4.78 s is The average A(1/[NO,]) / At from t= 4.78 s to t = 14.3 s is (3) Based on these data, the rate constant for this v order reaction is
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °CHI(g)½ H2(g) + ½ I2(g)the following data were obtained: [HI], M 0.573 0.287 0.144 7.20×10-2 seconds 0 520 781 912 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.573 M is s and when the starting concentration is 0.287 M is s.(2)The average rate of disappearance of HI from t = 0 s to t = 520 s is M s-1.(3)The average rate of disappearance of HI from t = 520 s to t = 781 s is M s-1.(4)Based on these data, the rate constant for this _______zerofirstsecond order reaction is M s-1.
In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)- →½ H2(g) + ½ I2(g) the following data were obtained: [HI], M seconds 1.48 0.740 0.370 0.185 750 2.25x103 5.25x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.48 M is 750 s and when the starting concentration is 0.740 M is 1500 S. (2) The average A(1/[HI]) / At from t = 0 s to t = 750 s is M-1 s-1. The average A(1/[HI]) / At from t 750 s to t = 2.25×103 s is M-1 s-1. (3) Based on these data, the rate constant for this 0 order reaction is M-1 s-1.
Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: step elementary reaction 1 NO (g) + Br₂ (g) → NOBr₂ (g) k₁ k₂ 2 NOBr₂ (g) + NO (g) → 2NOBr (g) Suppose also k₁ « k₂ . That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = k rate constant 010 X Ś