Choose the correct rate law for the following reaction: C6H5Cl + OH- → → C6H5OH + Cl- Ex [C6H5Cl]0 [OH-]0 init. rate/M•s–1 1 0.10 0.30 0.06 2 0.10 0.60 0.12 3 0.20 0.30 0.12
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Choose the correct rate law for the following reaction: C6H5Cl + OH- → → C6H5OH +...
consider the rate law below.
what is the value of the rate constant
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1. Consider the rate law below. What would happen to the rate constant if the initial concentration of B was doubled? Rate k [A][B]2 Use the following information to solve the question below. Initial Rate (M/s) Exp [A] M [BIM 1 0.20 M 0.000066 0.30 M 0.000132 2 0.20 M 0.60 M 0.000264 3 0.40 M 0.30 M What is the value of the rate constant?...
For the reaction of B with hydroxide ion, the following initial rate data are found: [B] (mol L-1) [OH-] (mol L-) Rate (mol L-4 s=1) 0.0100 1.0 x 10-4 1.2 x 10-3 0.0100 1.0 x 10-2 1.2 x 10-1 0.0025 1.0 x 10-2 3.0 x 10-2 What will the rate be when [Blo = 0.00100 M and [OH-] = 0.10 M in mol L-15-1? O A. 0.24 O B. 0.06 O C. 0.30 O D. 0.12 O E. 0.18
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7. You collect the following data for the reaction below. Write the rate law for the reaction, including a value and units fork from one of the trials data. Show calculations to find the order of each of the two reactants. Also estimate the reaction rate if the NO and O, concentrations were 0.30 and 0.75 M respectively. [12 pts.] NO(g) + 0,(s) - 2 NO, (g) [NO] (M) 0.10 0.35 0.10 10,1(M) 0.20...
Using the following data, determine the rate law and calculate k: rate = k[F2]x[ClO2]y Experiment [F2] (M) [ClO2] (M) Initial rate (M/s) 1 0.40 0.05 1.2 M/s 2 0.20 0.10 0.60 M/s 3 0.40 0.10 2.4 M/s
23. Given the following experimental data, find the rate law and the rate constant for the reaction: NO (8) + NO2 (g) + O2(g) → N2O(g) Run (NO), M (NO2), M (O2)., M. Initial Rate, Ms? 0.10 M 0.10 M 0.10 M 2.1 x 102 0.20 M 0.10 M 0.10 M 4.2 x 102 - NM + 0.20 M 0.30 M 0.20 M 1.26 x 102 0.10 M 0.10 M 0.20 M 2.1 x 102
Class Practice C152-02 Chapter 16 Practice 2 - Rate Law Consider a chemical reaction between compounds A and B that is first order with respect to A, first order with respect to B. and second order overall. From the information given below, fill in the blanks Initial Rate Initial (A) Initial [B] Experiment (Mrs) (M) (M) 1 4.0 x 100 .20 0.050 2 1 .6 x 102 0.050 3 3.28 10² 0.40 T Consider the following rate data for the...
5. The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) → 2SO42−(aq) + I3−(aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S2O82−](M) . [I−](M) . Initial Rate [M/s] 1 0.0300 0.0840 8.80 × 10−4 2 0.0300 0.0420 4.40 × 10−4 3 0.0600 0.0420 8.80 × 10−4 (a) Which of the following equations represents the rate law for this reaction? What is the...
Seat # Ver. K J. Quest. 6 (9 pts). The following initial rates were obtained for the reaction -120 kJ Δ Η 2C 2A +B [B] (M) 0.30 0.60 [A] (M) 0.20 Rate (M/s) 0.127 0.40 1.02 0.254 0.509 0.60 0.20 0.40 0.30 a. Determine the rate law for the reaction. b. Calculate the rate when B 0.40 M and A 0.65 M. a. With the aid of the rate law, propose a plausible two-step mechanism for the reaction. Label...
6. Consider the reaction X + Y → Z Initial Rate of Disappearance of X (M/s) [X] (M) [Y] (M) 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30 From the data in the table, obtained at 360 K, (a) determine the overall order of the reaction (b) determine the initial rate of disappearance of X when the concentration of X is 0.30 M and that of Y is 0.40 M. ________ M/s
Be sure to answer all parts. Consider the reaction X + Y Z Initial Rate of Disappearance of [X] (M) [Y](M) X (M/s) From the data in the table, obtained at 360 K, 0.053 0.10 0.50 (a) determine the overall order of the reaction 0.20 0.30 0.127 1.02 0.254 0.40 0.60 0.20 0.60 0.30 0.509 0.40 (b) determine the initial rate of disappearance of X when the concentration of X is 0.40 M and that of Y is 0.30 M....