ysn_/mMmrqent Veri...Bb LogoutMyProgrammingLabImported From IEITEC2110:Summer2...TunesToTube - Upl..Web Development.Publix App.O KINETICS AND EQUILIBRIUMUsing the Arrhenius equation to calculate k at one temperature fr..CiaThe rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E = 14.0 kJ/mol. If the rate constant of this-1reaction is 1.6x 10' MS-1at 134.0 °C, what will the rate constant be at 74.0 °C?Round your answer to 2 significant digits.-1-1x10CheckExplanation

The term Arrhenius equation in chemistry can be defined as the equation which is used to dependence…

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Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 53AP

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b) what is the velocity of a reaction when [S] = 20 mM, where Vmax = 100 umol/mL*sec, and 4 Km = 2mM? can you show me how he got 98 umol / mL*sec, very close to Vmx, as [S]>>Km, at zero order of the kinetics. step by step please
(a) Can an intermediate appear as a reactant in the firststep of a reaction mechanism? (b) On a reaction energyprofile diagram, is an intermediate represented asa peak or a valley? (c) If a molecule like Cl2 falls apart inan elementary reaction, what is the molecularity of thereaction?
Please include the reaction mechanism aswell
Suppose that for the reaction K + L------->M, you monitorthe production of M over time, and then plot the followinggraph from your data: (a) Is the reaction occurring at a constant rate from t = 0to t = 15 min? (b) Is the reaction completed at t = 15min? (c) Suppose the reaction as plotted here were startedwith 0.20 mol K and 0.40 mol L. After 30 min, an additional0.20 mol K are added to the reaction mixture.Which of the following correctly describes how the plotwould look from t = 30 min to t = 60 min? (i) [M] wouldremain at the same constant value it has at t = 30 min,(ii) [M] would increase with the same slope as t = 0 to15 min, until t = 45 min at which point the plot becomeshorizontal again, or (iii) [M] decreases and reaches0 at t = 45 min.
Some sulfuric acid is spilled on a lab bench. You can neutralizethe acid by sprinkling sodium bicarbonate on it and thenmopping up the resulting solution. The sodium bicarbonatereacts with sulfuric acid according to:2 NaHCO31s2 + H2SO41aq2¡Na2SO41aq2 +2 H2O1l2 + 2 CO21g2Sodium bicarbonate is added until the fizzing due to the formationof CO21g2 stops. If 27 mL of 6.0 M H2SO4 was spilled,what is the minimum mass of NaHCO3 that must be addedto the spill to neutralize the acid?
The reaction: H2 + I2 = 2HI has an Eactivation = 2000 J/mol. Suppose that it has K=7.5x10-5 M-1s-1 at T=700K, find K at T=800K.
Mention the two important features of solid catalysts and explain with thehelp of suitable examples.
Conventionally, we report reaction rates as absolute values (i.e., without reporting the sign). TrueFalse
Suppose that a reaction of stoichiometry A + B ----> Y + Z is believed to occur according to the mechanism: A ---k1---> X X ---k'1---> A X + B ---k2---> Y + Z Apply the steady-state treatment and obtain an expression for the rate. To what expressions does the general rate equation reduce if (explain your rationale in each case):The second reaction is slow ,the initial equilibrium being established very rapidly . b. If the second reaction is very rapid compared with the first reaction in either direction.
for the reaction A -> B where at t=0, t=20s, t=40s A=0.30 mol A=1.0mol A=0.54mol B= 0.46mol B=0.70mol calculate tge average appearance of B over the time interval from 0 -> 40s
The ha lf-lives for the forward and backward reactions of a reaction that is first-order in both directions are 24 ms and 39 ms respectively. Calculate the correspond ingre laxation time for return to equilibrium after a temperaturejump.
For a first order reaction Arightwards arrowB the following data is collected at 3000C. Use the data in the table to determine concentration of A at 84 s. Time (s) Concentration of A (M) 0.00 0.350 10.00 0.185 Hint: Integrated Rate equation in relation to first order reaction

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