10. The oxidation of iodide ion by hydrogen peroxide in an acidic solution is described by thebalanced equationH2O2(aq)+31(aq)+2H*(aq)¬I;'(aq)+2H2O(1)The rate of formation of the red triiodide ion, A[I3/At, can be determined by measuring the rateof appearance of the color (see the figure).Initial rate data at 25 C are as follows:ExperimentInitial [H2O2]Initial [I-]Initial Rate of Formationof [I3](M/s)10.1000.1001.15×1040.1000.2002.30×10¬40.2000.1002.30×10-4pts) What is the rate law for the formation of I;?ХаRate =ots)What is the value of the rate constant, k? (include correct units for k)DEGtarlo anmollo anm[AHON/C) What is the initial rate of formation of I3 when the initial concentration= 0.200 M and [I]= 0.600 M ? Include correct units.TSexTAHLNOFFTAN-ITANyxστηVASOxn-1ilvery gray metal and tolo

The given reaction is, H2O2(aq) + 3I-(aq) + 2H+(aq) → I3-(aq) + 2H2O(l) Suppose the rate law for the…

10. The oxidation of iodide ion by hydrogen peroxide in an acidic solution is described by the balanced equation soof H2O2(aq)+31(aq)+2H*(aq)¬I; (aq)+2H2O(1) The rate of formation of the red triiodide ion, A[I3/Ar, can be determined by measuring the rate of appearance of the color (see the figure). Initial rate data at 25 C are as follows: Initial Rate of Formation

10. The oxidation of iodide ion by hydrogen peroxide in an acidic solution is described by the balanced equation soof H2O2(aq)+31(aq)+2H*(aq)¬I; (aq)+2H2O(1) The rate of formation of the red triiodide ion, A[I3/Ar, can be determined by measuring the rate of appearance of the color (see the figure). Initial rate data at 25 C are as follows: Initial Rate of Formation

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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(1) The oxidation of ammonia produces nitrogen and water via the following reaction: 4 NH3(g) +3 02(g) → 2 N2(g) +6 H₂O(1) If rate of formation of H2O(7) is 3.0 mol/(L. s) is, (a) What is the rate of formation of Nitrogen gas? (b) What is the rate of disappearance of Ammonia gas?
Consider the reaction 5B1¯ (aq) + Br0, (aq) + 6H† (aq)→3B12 (aq) + 3H2O(1) The average rate of consumption of Br is 1.16×10-4 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval? Express your answer with the appropriate units.
Obtain the 2"-1 – 1 | T (п - 1)k. а"-1 relation between the order of the reaction (n), the reaction rate constant (k), the initial concentration (a), and the half-life (T).
a)A nickel catalyst is commonly used in the hydrogenation of ethylene. If the initial concentration of ethylene is 2.75 mol·L−1 and the rate constant for the reaction is 0.0018 mol·L−1·s−1, what is the rate of reaction if it follows a zero-order reaction mechanism? Express your answer to two significant figures. b)Determine the half-life for the reaction in Part B. Express your answer to two significant figures.
1. (a) The decomposition of SO2C12 is a first order reaction. SO2C12 (g) → SO2 (g) + Cl2 (g) i) Write the rate differential equation for the reaction. ii) Calculate the value of rate constant, k at 500K if 5.00 % SO2C12 decomposed in 6.75 mins. iii) Calculate the half-life for the decomposition.
Consider the following reaction: 2A + B + 3C. (a) Write an expression for the overall rate; (b) What are the rates at which A and B are consumed and generated if C is created at a rate of 0.015 M/min?
The gas phase reaction between hydrogen and iodine is proposed to occur as follows: step 1 fast: I =21 step 2 slow: H, + 2 I —2 HІ (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"[B]"... , where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =
The gas phase reaction between hydrogen and iodine is proposed to occur as follows: step 1: 12 →21 step 2: step 2 H₂ + 2 I (a) Identify the molecularity of each step in the mechanism. step 1 → 2 HI + (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + (c) Identify any intemediates in this mechanism. Intermediate: Enter formula. If none, leave box blank:
The following kinetic data were collected at 298 K for the reaction of ozone with nitrite ion, producing nitrate and oxygen: NO, (aq) +O,(g) NO, (aq) +0,(g) > Experiment [NO2 lo (M) [O3lo (M) Initial Rate (M/s) 1 0.0100 0.0050 25.0 0.0150 0.0050 37.5 3 0.0200 0.0050 50.0 0.0200 0.0200 200.0
The isomerization of methyl isonitrile (CH3NC) to acetonitrile(CH3CN) was studied in the gas phase at 215 °C,and the following data were obtained: (a) Calculate the average rate of reaction, in M/s, for thetime interval between each measurement. (b) Calculatethe average rate of reaction over the entire time of thedata from t = 0 to t = 15,000 s. (c) Which is greater, theaverage rate between t = 2000 and t = 12,000 s, or betweent = 8000 and t = 15,000 s? (d) Graph [CH3NC]versus time and determine the instantaneous rates in M/sat t = 5000 s and t = 8000 s.
The following data were obtained on the initial rates of a reaction of a d-metal complex in aqueous solution. What is (a) the order of reaction with respect to the complex and the reactant Y. (b) the rate constant? For the experiments (a) [Y] = 2. 7 mmol dm-3 and for experiments (b) ]Y] = 6.1 mmol dm-3[complex]/(mmol dm-3) 8.01 9.22 12.11v/(mol dm-3 s-1) (a) 125 144 190 (b) 640 730 960
The reaction described by the following equation: 21-(aq) + H;O2(aq) + 2H*(aq) → I:(aq) + 2H;O(aq) has an experimental rate law (v) = k[I][H2O2]. Suggest a plausible mechanism for this reaction, and identify the rate-determining step.