Given a reaction that occurs through the collision of A and B. Calculate the rate law, and showwhen it behaves as a diffusion-controlled reaction.(- k,' + A + B{l -k+А + в -k, — АВP

A chemical reaction happens when the two or more substrates are combined together to form an…

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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

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2) For a first order reaction the concentration of the reactant A changes with time according to the following table: t(s) [A] (M) 0 0.110 200 0.073 400 0.048 600 0.032 1000 0.014 A) Find the rate constant k graphically? Prove your answer mathematically? B) Find the concentration of A at 100 s graphically? Prove your answer mathematically?
If the rate law for the reaction bewteen NO and O2 is Rate = k[NO]3[O2] the units of k are M-1s-1 Is this true or false?
Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) O₂(g) + 0(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁ »k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate constants k.1 and k-2 for the reverse of the two elementary reactions in the mechanism. = 0 k = 00 X 5 S ?
a The rate law for the reaction rogress 2NOBr(g) → 2NO(g) + Br2 (g) at some temperature is ΔΙΝΟΒ Rate = - = k[NOB1]² At If the half-life for this reaction is 2.00 s when [NOB1]o= 0.90 M, calculate the value of k for this reaction. k = L/mol·s Submit
The rate constant for this first‑order reaction is 0.0240 s−1 at 400 ∘C. A⟶products After how many seconds will 21.7% of the reactant remain? t=
Given- H2S (g) + O2 (g) → H2O (g) + S8 (g)-Write the expression of the rate in terms of the concentration of eachreactant and product over time.-If the rate of formation of S8 is 0.078 M/s, what is the rate ofdisappearance of H2S?
A chemical engineer is studying the rate of this reaction. 2N2O5(g)>>>2N2O4(g)+ O2(g) She fills a reaction vessel with N, O, and measures its concentration as the reaction proceeds. Here's a graph of her data: What is the half life of the reaction? Suppose the rate of the reaction is known to be first order in N2O5 Calculate the value of the rate constant k. Predict the concentration of N2O5 in the engineer's reaction vessel after 8.5 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in N2O5.
The decomposition reaction of ammonia gas (NH3) into hydrogen gas (H2) and nitrogen (N2) with a Pt catalyst is a zero order reaction at a temperature of 1130 K (i) rate of reaction = rate constant,(ii) reaction rate depends on ammonia concentration,(iii) the rate of decomposition of ammonia becomes constant when the ammonia has completely reacted,(iv) an increase in gas pressure will change the rate of the reaction. A. (ii) and (iv)B. (i) and (ii)C. (i), (ii) and (iii)D. (ii), (iii) and (iv)E. (i), (iii) and (iv)
The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, ? , of a particular gaseous reaction as 9.20×10−10 cm3⋅molecule−1⋅s−1 at 298 K .Convert the rate constant to units of M−1⋅s−1 .?=5.5×1011M−1⋅s−1Convert the rate constant to units of Torr−1⋅s−1 .?=Torr−1⋅s−1.
The following mechanism has been proposed for the atmospheric destruction of ozone, O3 (g):O3 (g) + NO (g) --> O2 (g) + NO2 (g) (slow)NO2 (g) + O (g) --> NO (g) + O2 (g) (fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.
Consider the following mechanism for the formation of nitrogen dioxide: 2 NO(g) N2O2(g) (1) N,O2(9) + O2(9) → 2 NO2(g) (2) Write the chemical equation of the overall reaction: yes 0,0,.. Are there any intermediates in this mechanism? no ? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one.
Write the reaction rate equation and identify the order of the reaction: Chemical Equation Type of Order Reaction Rate H2(g) + I2(g) => 2HI(g) NO(g) + O3(g) => NO2(g) + O2(g) 4OH(G) + H2S(g) => SO2(g) + 2H2O(aq) + H2(g)

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Given a reaction that occurs through the collision of A and B. Calculate the rate law, and show when it behaves as a diffusion-controlled reaction. (-k' → A + B A + B - k → AB l-k+ P