The following rate information wascollected for the reaction:2MnO4 (aq) + 5CIO3 (аq) + 6H*> 2Mn²+ (aq) + 5 CIO4 (aq) +(aq)-->3H20(1)Exp. # [MnO4][H*][CIO3]Initial Rate (M/s)10.100 М0.100 MО.100 М5.20 х 10-30.250 M0.100 MО.100 М3.25 х 10°230.100 MО.300 М0.100 М1.56 x 10-240.100 М0.100 M0.200 M7.35 x 10-3What is the rate law (don't forget tofind the value of k as well)? (showwork)

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The following rate information was collected for the reaction: 2MNO4 (aq) + 5CIO3 (aq) + 6H+ --> 2MN2+ (aq) + 5 CIO4" (aq) + (aq) 3H20(1) Exp. # [MnO4] [H*] [CIO3] Initial Rate (M/s) 1 0.100 M 0.100 M 0.100 M 5.20 х 10-3 0.250 M 0.100 M 0.100 M 3.25 х 10°2 3 0.100 M 0.300 M 0.100 M 1.56 x 10-2 4 0.100 M 0.100 M 0.200 M 7.35 x 10-3 What is the rate law (don't forget to find the value of k as well)? (show work)

The following rate information was collected for the reaction: 2MNO4 (aq) + 5CIO3 (aq) + 6H+ --> 2MN2+ (aq) + 5 CIO4" (aq) + (aq) 3H20(1) Exp. # [MnO4] [H*] [CIO3] Initial Rate (M/s) 1 0.100 M 0.100 M 0.100 M 5.20 х 10-3 0.250 M 0.100 M 0.100 M 3.25 х 10°2 3 0.100 M 0.300 M 0.100 M 1.56 x 10-2 4 0.100 M 0.100 M 0.200 M 7.35 x 10-3 What is the rate law (don't forget to find the value of k as well)? (show work)

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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A chemical engineer is studying the rate of this reaction. H_CO, (aq) + H,O (aq)+CO,(aq) He fills a reaction vessel with H₂CO3 and measures its concentration as the reaction proceeds. Here's a graph of his data: [H₂CO₂] (M) 08- 04- 02+ 0+ 02 0.6 1 (s) What is the half life of the reaction? 0.8 Use this graph to answer the following questions: Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in H₂CO3. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of H₂CO3 in the engineer's reaction vessel after 2.00 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in H₂CO3. Round your answer to 2 significant digits. = k = 0 0₁ [H.CO,] = M Ox 0.0 X 4
A) Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) What is the rate law for this reaction? Group of answer choices rate = k [H+][NO3-] rate = k [H+]10[NO3-]2[Zn2+]4[N2O] More information is needed to determine this. rate = k [H+]10[NO3-]2 B) Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) If the rate of H+ disappearance is 0.0250 M/min, what is the rate of Zn2+ appearance? Group of answer choices 0.0100 M/min 0.00100 M/min 0.0250 M/min 0.0625 M/min
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Using the data in the table, calculate the rate constant of this reaction. k= A+B C+D Trial 1 2 3 Units [A] (M) 0.260 0.260 0.364 [B] (M) 0.350 0.945 0.350 Rate (M/s) 0.0167 0.122 0.0234
REACTION A +B + C Products [B](M) 1.0 2.0 1.0 1.0 Rate(M/s) 1.0E-4 4.0E-4 2.0E-4 2.0E-4 Trial 1 [A](M) [C](M) 1.0 0.010 1.0 0.010 3 1.0 0.020 2.0 0.010 Using the data in the table and the rate law below, identify the reaction order with respect to each reatant. Rate = k[A]M[B]^[c]P (Rate = k times [A] to the mth power times [B] to the nth power times [C] to the pth power) %3D
The data given below refers to the reaction: A(aq) + 2B(aq) --> D(aq) + C (ag) What rate law is consistent with this kinetic data? Trial [A], M [B], M Rate of formation of D, M/s 0.100 0.100 3.00 x 10 - 4 0.300 0.300 9.00 x 10 - 4 3 0.100 0.300 3.00 x 10 - 4 4 0.200 0.400 6.00 x 10 - 4 A Rate = k B Rate = k[A] Rate = k[B] Rate = k[A][B] O A O B O C O D
Use the data presented in the table to determine the rate equation for the hypothetical reaction shown. A(g) + 2B(g) + 3C(g) [Math Processing Error] D(g) + 2F(g) Exp {A} (M) {B} (M) {C} (M) initial rate (M/min) 0.0025 0.0025 0.0025 3.16x10-11 0.0025 0.0050 0.0025 1.27x10-10 3 0.0050 0.0050 0.0025 1.27x10-10 4 0.0100 0.0100 0.0050 4.06x10-9 What is the reaction order with respect to A? What is the reaction order with respect to B? What is the reaction order with respect to C? Enter each of your answers numerically as integers or fractions (ex: 0, 1/2, 1, 3/2, 2, 3, etc). Hint: Determining the order of one of the reactants will be difficult. Determine the order of the two easy reactants first, then use that information in determining the difficult one.
3
2. Consider the reaction A+2B C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [v] (M) (M) (M/s) [B] Rate Trial 1 0.10 0.050 6.0x10-4 0.10 0.100 1.2x10-3 3 0.20 0.050 2.4x10-3 Part B Provide
A: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) What is the rate of Zn2+ formation if its concentration rises from 0.00 to 0.069 M in 2 minutes and 12 seconds? Group of answer choices 0.031 M/s 2.1 x 10-3 M/s 1.3 x 10-4 M/s 5.2 x 10-4 M/s B: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) If the rate of H+ disappearance is 0.0250 M/min, what is the rate of Zn2+ appearance? Group of answer choices 0.0100 M/min 0.00100 M/min 0.0250 M/min 0.0625 M/min
E. For the reaction A+B+C→D+EA+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A][A](MM) [B][B](MM) [C][C](MM) Initial rate(M/sM/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4