For the reaction t (s) [H*] (M) 2.32 CHJОнаq) + H*аq) + CI Taq) — сH C{aq) + H200) 30.0 2.10 the value of [H+ was measured over a period of time. Given the data in the table, find the average rate of disappearance of H*(aq) for the time interval between each measurement. 65.0 1.98 123.0 1.81 Interval: 0 s to 30.0 s reaction rate: M/s Interval: 30.0 s to 65.0 s reaction rate: M/s Interval: 65.0 s to 123.0 s reaction rate: M/s What is the average rate of appearance of CH Cl(aq) for the same time intervals? Interval: 0 s to 30.0 s reaction rate: M/s Interval: 30.0 s to 65.0 s reaction rate: M/s Interval: 65.0 s to 123.0 s

For the reaction t (s) [H] (M) 2.32 CHJОнаq) + Hаq) + CI Taq) — сH C{aq) + H200) 30.0 2.10 the value of [H+ was measured over a period of time. Given the data in the table, find the average rate of disappearance of H*(aq) for the time interval between each measurement. 65.0 1.98 123.0 1.81 Interval: 0 s to 30.0 s reaction rate: M/s Interval: 30.0 s to 65.0 s reaction rate: M/s Interval: 65.0 s to 123.0 s reaction rate: M/s What is the average rate of appearance of CH Cl(aq) for the same time intervals? Interval: 0 s to 30.0 s reaction rate: M/s Interval: 30.0 s to 65.0 s reaction rate: M/s Interval: 65.0 s to 123.0 s

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) A study was made of the effect of hydroxide ion, OH–, concentration on the rate for the following reaction: I–(aq) + OCl–(aq) ----------------> IO–(aq) + Cl–(aq) Experimental data: [I] [OCl–] [OH–] Rate M/sec 0.0013 0.012 0.1 9.4 x 10-3 0.0026 0.012 0.1 18.7 x 10-3 0.0013 0.006 0.1 4.7 x 10-3 0.0013 0.018 0.1 14.0 x 10-3 0.0013 0.012 0.05 18.7 x 10-3 0.0013 0.012 0.2 4.7 x 10-3 0.0013 0.018 0.2 7.0 x 10-3 Determine the rate law and the value of the rate constant, k.
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For the following reaction 4 experiments have been run and the data collected is in the following table: 2 MnO, (aq) + 5 H,C,0, (aq) + 6 H* (aq) 2 Mn2+ (aq) + 10 CO2 (g) + 8 H,0 (1) Experimen [MnO,], M [H,C,O,], M [H*], M Rate, M/s t 1 0.2410 0.3470 0.2690 0.1147 2 0.3260 0.6210 0.2270 0.2776 3 0.5630 0.5740 0.7420 0.4431 4 0.2410 0.3470 0.3840 0.1147 0.4140 0.5740 0.5610 0.3258 6. 0.3260 0.4930 0.4910 0.2203
An iodine clock experiment was performed and the following data was recorded. Determine the initial concentration (mM) of thiosulfate (limiting reactant) in the reaction and calculate the initial rate (mM/s) for the reaction. 3 I- (aq) + 2 H* (aq) + H2O2 (aq) – I3^ (aq) + 2 H2O ( I 13(aq) + 2 S₂O32- (aq) → 31¯ (aq) + S406²- (aq) 13(aq) + starch intense blue color Concentration of iodide solution Concentration of thiosulfate solution Concentration of hydrogen peroxide solution Volume of iodide solution used Volume of thiosulfate solution used Volume of hydrogen peroxide solution used Volume of DI water used Time APERTANTORARIASENAMEN 230.0 mM 40.2 mM 352.0 mM 20.0 mL 2.0 mL 13.0 mL 5.0 mL 33.5 s
Using the data in the table, determine the rate constant of the Trial [A] (M) [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.340 0.340 0.0106 A + 2B C + D 2 0.340 0.680 0.0106 3 0.680 0.340 0.0424 Units k = M-s-1 M-'s-1 M-2s-1 s-1
For the reaction 4A(g) + 3B(g) → 2C(g) The following data were obtained at constant temperature: Experiment Initial [A](mol/L) Initial [B](mol/L) Initial Rate(mol/L · min) 1 0.100 0.100 5 2 0.300 0.100 45 3 0.100 0.200 10 4 0.300 0.200 90 Pick the best expression for the rate law for the reaction: k[A]2[B] Correct Calculate k (using the data from the table),
Using the data in the table, determine the rate constant of Trial [A] (M) [B] (M) Rate (M/s) the reaction and select the appropriate units. 1 0.280 0.200 0.0163 A +2B C+ D 0.280 0.400 0.0163 0.560 0.200 0.0652 Units k =
Consider this initial rate data at a certain temperature in the table for the reaction [OCI-], [I]o [OH-]o Initial rates OH (aq) OCI (aq) + I (aq) OI (aq) + Cl¯(aq) Trial (М) (М) (M/s) (М) 1 0.00185 0.00185 0.450 0.000494 0.00185 0.00324 0.450 0.000864 3 0.00350 0.00185 0.621 0.000676 0.00324 0.653 0.000596 4 0.00185
3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096
An experiment was carried out to investigate the effect of concentration on the reaction: BrO3(aq) + 5 Br (aq) + 6 H* (aq) = 3 Br₂ (1) + 3 H₂O (1) The following data was obtained: Initial [BrO3] Initial [Br] Initial [H*] Initial Rate Trial (mol/L) (mol/L) (mol/L) (mol/L's) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) Deduce and state the rate law equation for this reaction. Show your process/reasoning. b) Calculate the value of k, the rate constant with correct units.
For the rate expression below, determine the exponents x and y for the following data. Rate = k [A] [B]Y Trial [A] M 1 2 3 4 0.10 Hint 0.20 0.10 0.30 x=1, y=0 x=0, y=1 Ox=1, y=2 x= 1, y=1 x=2, y=1 [B] M 0.20 0.20 0.10 Initial rate 4.6x10-2 9.2x10-² 2.3x10-2 0.30 1.4x10-1
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