1. A reaction between A and B was found to give the following: Trial 1 2 3 4 [A] mol/L 0.142 0.426 0.246 0.142 2 A+3B C+2D [B] mol/L 0.277 0.277 0.246 1.108 Initial Rate of Reaction mol/(Los) 1.08 × 10-4 9.75 × 10-4 2.89 × 10-4 4.33 × 104 From the data, determine a rate equation for the reaction. Please provide a value for the rate constant with proper units. rate= K[A[B²] 207 a

1. A reaction between A and B was found to give the following: Trial 1 2 3 4 [A] mol/L 0.142 0.426 0.246 0.142 2 A+3B C+2D [B] mol/L 0.277 0.277 0.246 1.108 Initial Rate of Reaction mol/(Los) 1.08 × 10-4 9.75 × 10-4 2.89 × 10-4 4.33 × 104 From the data, determine a rate equation for the reaction. Please provide a value for the rate constant with proper units. rate= K[A[B²] 207 a

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.2CE: Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of...

See similar textbooks

Similar questions

The kinetic data shown below were observed for the reaction: BF3 (g) + NH3 (g) ---------> F3B·NH3 (g) Trial # [BF3] (mol/L) [NH3] (mol/L) Rate (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 What is the rate constant for this experiment?
Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+DA+B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.3600.360 0.2200.220 0.01600.0160 2 0.3600.360 0.5940.594 0.1170.117 3 0.5760.576 0.2200.220 0.02560.0256
Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.400 0.370 0.0216 2 0.400 0.962 0.146 3 0.600 0.370 0.0324 ?=
Table 2: Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 help me with this part please, and show me all steps Order with respect to H2O2: Order with respect to KI:
Table 2: Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 Please help me with this part, and please show me all steps Order with respect to H2O2: Order with respect to KI:
Consider the chemical reaction described by 2A(aq) ⇌ D(aq)with rate constants k1 and k-1. If k1 = 5.9×10-5 Lmol-1s-1 and Keq = 0.27 what is k-1 for a solution originally prepared with [A]0 = 0.123 molL-1 and [D]0 = 0?
Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?] (?) [?] (?)[) Rate (M/s) 1 0.370 0.390 0.0234 2 0.370 0.936 0.135 3 0.592 0.390 0.0374 ?= ? units= ?
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+DA+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.2100.210 0.3000.300 0.02210.0221 2 0.2100.210 0.6000.600 0.02210.0221 3 0.4200.420 0.3000.300 0.08840.0884
Pls do fast within 5 min .. I will give u 3 like for sure The reaction of an aryl amine with nitrite in the presence of perchlorate produces a diazonium salt. The initial rate of this reaction was measured using UV spectrometry at 25°C, at fixed initial concentrations of the aryl amine and perchlorate, but varying the initial concentration of nitrite. [nitrite]0 / mol dm−3 0.06 0.04 0.02 0.01 Initial rate / 108 mol dm−3 s −1 39.0 18.0 5.0 1.5 Using the table of data show that the reaction proceeds according to the rate law rate = k1[nitrite] + k2[nitrite]2 and calculate values for the rate constants.
I monitor the reaction of Compound B with a large excess of NaOH at 298 K, and get the following results for its absorbance over time: Time (seconds) Absorbance (no units) 0 0.4555 10 0.3857 20 0.3178 30 0.2457 40 0.2011 50 0.1798 60 0.1304 On the basis of these numbers and a spreadsheet program, answer the following question: What is the most-likely order of Compound B in its reaction with NaOH? a. 0 b. 4 c. 1 d. 3 e. 2
Determine the missing initial rate: 2N2O5 → 4NO2 + O2 [N2O5] Initial rate (Ms-1) 0.093 4.84x10-4 0.084 4.37x10-4 0.224 ??
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.340 0.210 0.0204 2 0.340 0.420 0.0204 3 0.680 0.210 0.0816 ?=