2NO(g) + O₂(g) → NO2(g)Conc. NO, mol/LExp. 1 4.3 x 10-2Exp. 2 4.3 x 10-2Exp. 3 8.6 x 10-²Exp. 4 0.63Conc. 02, mol/L2.4 x 10-²4.8 x 10-29.6 x 10-²5.4 x 10-³Initial Rate8.0 x 10³ mol/(L.s)1.6 x 102 mol/(L.s)0.13 mol/(L.s)?a What is the experimental rate law for the reaction above?(Use k for the rate constant.)Rate law = K[NO]²[0₂]✔Co-The reaction is first order in O₂ because the rate doubled with a dosecond order in NO because the rate increased by a factor of 8 whRate = k[NO] ² [0₂]b What is the initial rate of the reaction in Experiment 4?Initial rate=mol/(L.s)

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Answered: b What is the initial rate of the…

Chemistry

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Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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nder [reactant), Treactant]," rate, rate; What is the reaction order with respect to A? (A), mol/L (B), mol/L rate, mol/(L-min) Trial 1 0.931 0.549 0.0781 Trial 2 1.86 0.549 0.0781 Trial 3 0.931 1.10 0.312 Trial 4 0.466 0.829 0.178 Rate = k(A]ordera B]arderb 2
For the reaction: BrO3-(aq) + 5Br (aq) + 8H*(aq) → 3Br2(/) + H201) The initial rate of the reaction has been measured at the reactant concentration show: Trial [BrO;] (mol/L) 1 [H'] [Br ] Initial rat (mol/L) (mol/L) (mol/L-s) 0.10 0.10 0.10 8.0 0.20 0.10 0.10 16 0.10 0.20 0.10 16 4 0.10 0.10 0.20 32 The value for k will be: A L/mol.s Ouestion 13 (1 23
Question 12 of 19 Submit What is the half-life for a particular reaction if the rate law is rate = (1201 min )[A]? min 1 2 3 4 6. C 8 9. +/- х 100 7.
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.
(35) The following data were obtained for the hypothetical reaction 2A + B → products. [A]o (M) [B]o (M) Initial Rate (M/s) 0.2 0.1 0.2 0.2 20 0.6 0.1 15 What is the overall order of this reaction? а. 4 b. ½ с. 0 d. 3 е. 1
A+B- -AB Trial (A] (M) (B] (M) Rate (M/s) 1 0.200 0.200 2.00 x 102 0.400 0.200 8.00 x 102 0.200 0.400 4.00 x 102 What is the rate constant for the reaction above? 2.
Use the following data table to answer the following questions. Experiment Concn. of A (M) Concn. of B (M) Initial rate (M/s) 1 0.10 0.010 1.2e-3 2 0.10 0.040 4.8e-3 3 0.20 0.010 2.4e-3 d. The rate constant of the reaction is e. The rate of reaction when concentration of A and B are 0.15M and 0.075M is
2) The rate law for a certain reaction is Rate = k[A]2. If the concentration of A is halved, the rate of the reaction will decrease by a factor of ... A.1 B.8 С.2 D.4 E.16
A researcher was analyzing a data set from an initial rate experiment for the reaction of baking soda and vinegar at 25°C. NaHCO3 + HC2H3O2 CO2 + H20 + NaC2H3O2 Experiment [NaHCOgl. M[HC2H3O2), Mrate (M/s) 3.000 1.500 0.750 0.400 0.400 0.0360 0.0180 3 0.400 0.0090 The researcher suggested the following rate law based on these results: rate = k[NaHCO), with a k 0.012 s. Do you agree with the researchers conclusion, why or why not. O CHEM1212
In a particular reaction, BrO3- + 5 Br- + H3O+ → 3 Br2 + 9 H2O , the following table below is completed with the initial concentrations of each reactant and the initial rate for each trial. 1.) Write the rate expression for this reaction. (HINT: rate = -Δ[rcts]/Δt = +Δ[pdcts]/Δt ... ) 2.) Write the rate law for this reaction. (HINT: rate = k [rcts]x ... ) 3.) What is the overall order for this reaction? 4.) What is the rate constant (k) for this reaction? Extra Credit: Calculate the rate of this reaction when [BrO3-] = 0.50 M, [Br-] = 0.25 M, and [H3O+] = 0.35 M.
* 97% 7:58 PM Wed Feb 12 х Unanswered •1 attempt left • Due on Feb 13 Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B]^0 [C] The unit of k is sec/M 1/M^3-sec 1/M^2-secc. 1/M^4-sec M^3/sec Submit
Question 7 of 8 Submit A reaction has a rate law of Rate = (1.25 M-1s-1)[A][B]. What is the rate of the reaction %3D if [A] = 0.301 M and [B] = 0.280 %3D %3D M? |M/s 1 4 5 6 C 7 8 9. +/- x 100

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b What is the initial rate of the reaction in Experiment 4? Initial rate= mol/(L.s)