In a study of the gas phase decomposition of hydrogen peroxide at 400 °C H,O2(9H20(g) +¾ O2(g) the concentration of H2O2 was followed as a function of time. It was found that a graph of 1/[H2O2] versus time in seconds gave a straight line with a slope of 0.969 M-1 s-l and a y-intercept of 7.09 M!. Based on this plot, the reaction is | ] order in H2O2 and the rate constant for the reaction is |

In a study of the gas phase decomposition of hydrogen peroxide at 400 °C H,O2(9H20(g) +¾ O2(g) the concentration of H2O2 was followed as a function of time. It was found that a graph of 1/[H2O2] versus time in seconds gave a straight line with a slope of 0.969 M-1 s-l and a y-intercept of 7.09 M!. Based on this plot, the reaction is | ] order in H2O2 and the rate constant for the reaction is |

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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Many chemical reactions follow the law which states that the velocity of the reaction is proportional to the difference between the initial concentration of the reagent and the amount transformed at any time. dx 3D k (а — х), di 0 < x < a Where a is the original concentration and x is the amount transformed at time t. If a=10 and x = 4 after 2 minutes, find the amount left after 5 minutes.
Hydrogen peroxide and the iodide ion react in acidic solution as follows: H2O2 (ag) + 31 (aq) + 2H† (ag) → I3 (aq) + 2H2O(1) The kinetics of this reaction were studied by following the decay of the concentration of H2O2 and constructing plots of In[H2 O2] versus time. All the plots were linear and all solutions had [H2O2], = 8.0 x 10-4 mol/L. The slopes of these straight lines depended on the initial concentrations of I¯ and H+. The results follow: I], (mol/L) [H*], (mol/L) Slope (min) 0.1000 0.0400 -0.120 0.3000 0.0400 -0.360 0.4000 0.0400 -0.480 0.0750 0.0200 -0.0760 0.0750 0.0800 -0.118 0.0750 0.1600 -0.174 The rate law for this reaction has the form -d[H2O2] (kı + k2 [H*])[I¯]™ [H2O2]" Rate = dt a Specify the orders of this reaction with respect to [H2O2] and [I¯]. п %3 т —
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The specific rate constant for the first-order decomposition of -1 N₂O5 (9) to NO2 (g) and O₂ (g) is 7.48 × 10-³ s¯ at a given temperature. Find the length of time required for the total pressure in a system containing N₂O5 at an initial pressure of 0.110 atm to rise to 0.150 atm . Express your answer using two significant figures. VE ΑΣΦ t = Submit Part B t = Submit Request Answer Find the length of time required for the total pressure in a system containing N₂O5 at an initial pressure of 0.110 atm to rise to 0.220 atm . Express your answer using two significant figures. ΨΕ ΑΣΦ Part C Request Answer ? Find the total pressure after 120 s of reaction. S S
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The decomposition of gaseous ozone 2 03 → 3 02, exhibits a rate law given by - d[O]] / dt = k [0;J / [0] Show that this rate law follows from the mechanism k1 O3 F k2 (1) 0 + O2 (2) 03 + 0 k3 >2 02 On the supposition that k2 >> k3. What is the resulting expression for k?
The following data were obtained for the reaction 2C102 (ag) + 20H (ag) → Cl0; (ag) + C102 (ag) + H,0(1) A[CIO2] where Rate = - At [C102]o (mol L) [OH ], (mol L) Initial Rate (molL·s) 0.0750 0.150 1.94 x 10-1 0.150 0.150 7.76 x 10-1 0.150 0.0750 3.88 x 10-1 a Determine the rate law. (Use k for the rate constant.) Rate = k[ClO,][OH] b Determine the value of the rate constant. Rate constant = 2.30x1 / L²/mol? - s c What would be the initial rate for an experiment with [CIO2], = 0.140 mol/L and [OH], = 0.0668 mol/L? Rate = mol/L·s
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