Consider the following elementary reaction: NO2(9) +F2(9) → NO,F(g) +F(g) Suppose we let k, stand for the rate constant of this reaction, and k_, stand for the rate constant of the reverse reaction. -1 Write an expression that gives the equilibrium concentration of F, in terms of k, k_1, and the equilibrium concentrations of NO,, NO,F, and F.

Consider the following elementary reaction: NO2(9) +F2(9) → NO,F(g) +F(g) Suppose we let k, stand for the rate constant of this reaction, and k_, stand for the rate constant of the reverse reaction. -1 Write an expression that gives the equilibrium concentration of F, in terms of k, k_1, and the equilibrium concentrations of NO,, NO,F, and F.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 96QAP: Consider the following energy diagram (not to scale) for the reaction. 2CH3(g)C2H6(g) (a) What is...

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Consider the following energy diagram (not to scale) for the reaction. 2CH3(g)C2H6(g) (a) What is the activation energy of the forward reaction? (b) At what point would 2CH3 (g) appear? (c) What is H for the reaction? (d) What is the activation energy of the reverse reaction? (e) At what point would C2H6 certainly be found? (f) What is any species at point C called?
a. Using the free energy profile for a simple one-step reaction, show that at equilibrium K = kf/kr, where kf and kr, are the rate constants for the forward and reverse reactions. Hint: Use the relationship G = RT ln(K) and represent kf and kr, using the Arrhenius equation.(K=AeEa/RT) b. Why is the following statement false? A catalyst can increase the rate of a forward reaction but not the rote of the reverse reaction.
Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
A. For a certain reaction, Kc = 4.48×106 and kf= 4.10×10−2 M−2⋅s-1 . Calculate the value of the reverse rate constant, kr, given that the reverse reaction is of the same molecularity as the forward reaction. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1nclude ⋅⋅ (multiplication dot) between each measurement. B. For a different reaction, Kc = 97.7, kf=3.00×10^3s−1 and kf=3.00×10^3s−1 , and kr= 30.7 s−1. Adding a catalyst increases the forward rate constant to 1.37×106 s−1s−1 . What is the new value of the reverse reaction constant, kr, after adding catalyst? Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1 include ⋅ (multiplication dot) between each measurement.
For a certain reaction, Kc�� = 9.80×10−10 and kf=�f= 2.59×10−5 M−2⋅s−1�−2⋅s−1 . Calculate the value of the reverse rate constant, kr�r, given that the reverse reaction is of the same molecularity as the forward reaction. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1�−2⋅�−1 include ⋅⋅ (multiplication dot) between each measurement. View Available Hint(s) For a different reaction, Kc�� = 5.40×102, kf=8.96×103s−1�f=8.96×103s−1 , and kr=�r= 16.6 s−1s−1 . Adding a catalyst increases the forward rate constant to 2.05×106 s−1s−1 . What is the new value of the reverse reaction constant, kr�r, after adding catalyst? Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1�−2⋅�−1 include ⋅⋅ (multiplication dot) between each measurement. View Available Hint(s)
Find the rate constant (k) for reaction mixture 1
Consider the following elementary reaction: N2O(g) -> N2(g) + O(g) Suppose we let k1 stand for the rate constant of this reaction, and k-1 stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of N2O in terms of k1, k-1, and the equilibrium concentrations of N2 and O
Each step represents an elementary reaction. Step1. A + 2B ↔ C (fast equilibrium, k1 and k-1) Step2. C + D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law. *e. Use the Steady-Sate Approximation to obtain the rate law.
Each step represents an elementary reaction.Step1. A + 2B ↔ C (fast equilibrium, k1 and k-1)Step2. C + D → E (slow, k2) *c. Find the rate-determining step (RDS) and express the rate law.d. Use the Pre-Equilibrium Approximation to obtain the rate law.*e. Use the Steady-Sate Approximation to obtain the rate law.
The following are Biophysical Chemistry Questions: When we are determining the equilibrium affinity (K) for a binding reaction or the rate constant (k) for a reaction, why do we make multiple measurements? Why is it useful to put one (or more) reagents in great excess of the other (for equilibrium analysis or kinetic analysis?) Why do you start learning about heat and work in thermodynamics witht the ideal gases instead of chemical reactions?
At a temperature of 700 K, the forward and reverse rate constants for the reaction 2HI <=> H2 + I2 are kf = 1.8 * 10-3 M-1 s-1 and kr = 0.063 M-1 s-1. Is the forward reaction endothermic or exothermic if the rate constants for the same reaction have values of kf = 0.097 M-1 s-1 and kr = 2.6 M-1 s-1 at 800 K?
In an experiment, you have a protein (p) that is able to bind to substrates x and y to form px and pxy. substrate y is dependent upon the binding of x, so py is not capable of forming. A. Form a chemical equation that describes the equilibrium of the reaction. Please label rate constants above the reation arrows. B. Using your previous answer, come up with an expression for {px} at equilibrium. C. Form an expression that defines the amount of {px} as a percentage. include {p}, {px} {pxy} in your answer.