Question 40 of 49Find the value of k for the rate law:Where the rate = 4.0*x 10-³ M/s, NO=0.45M and H+=1.15MA) 0.000932 1/M²sB) 0.00773 1/M²sC) 0.00207 1/M²sD) 0.0172 1/M²srate = k [NO]²[H+*]⁰E) 0.0198 1/M²s

Answered: Image /qna-images/answer/bb051e7b-bb42-4f8c-b09f-505ec515868f.jpg

Answered: Find the value of k for the rate law:…

Science

Chemistry

Find the value of k for the rate law: rate = k [NO]³[H]⁰ Where the rate = 4.0*x 10³ M/s, NO=0.45M and H=1.15M

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...

See similar textbooks

Related questions

Q: Consider this reaction: CICH,CH,CI (g) - CH,CHCI (g) + HCI (g) At a certain temperature it obeys…

A: Please find your solution below : A first order reaction is a chemical reaction in which the Kinetic…

Q: The reaction A → B + C is known to be zero order in A with a rate constant of 5.0 × 10–2 mol/L·s at…

A: A multiple choice question about zero order reaction, which is to be accomplished.

Q: NO2CI(g) + NO(g) 108 and E, is 28.9 kJ/mol. The rate equation is -----> NO2(g) + ONCI(g) A is 8.3 x…

A: Given- A=8.3×108 Ea=28.9kJ/mol =28.9 ×1000 = 28900 J/mole Rate constant of reaction=? There is…

Q: If the rate law for a process is rate=k[A]^2 [B], and [A]=0.7085 and [B]=0.1211, determine the rate…

A: Given :Rate = k [A]2 [B][A] = 0.7085 [B] = 0.1211We need to determine the rate as a multiple of k

Q: Consider the reaction described by the equation C,H,Br, (aq) +31 (aq) C,H(g) + 2 Br (aq) +15 (aq)…

A: Given: Rate law of reaction: Rate = K[C2H4Br2][I-] Rate constant, K = 0.00447 M-1s-1. And the table…

Q: Ozone decomposes to form oxygen molecules and oxygen atoms, O3(g)→O2(g) + O(g), in the upper…

Q: A certain reaction has the following general form: aA + bB At a particular temperature and [A], =…

A: From the graph we conclude that the given reaction is second order kinetics in which a=2.

Q: For which of these rate laws is the half-life independent of initial concentration? rate = k…

A: The rate law for which the half-life is independent of initial concentration has to be given.

Q: A reaction obeys the following rate law: Rate = k [A]2 (k = 0.00813 M¹5¹) Initially, a vessel…

Q: HELP Calculation of order of reaction Nitrogen di-oxide reacts with carbon monoxide to exchange…

Q: The rate law for the reaction A + B - 3C was determined to be v = k[AJ°[B]° at 20°C. If the reaction…

Q: H2SEO3 (ag) + 6 Ir(ag) + 4 H* (ag) –→ Se(s) + 2 13 (ag) + 3 H20 (I) The following data are obtained…

Q: Consider the reaction described by the equation The rate law is C₂H, Br, (aq) +31(aq) C₂H₂(g) + 2 Br…

Q: Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate…

Q: rate law

Q: Consider the following reaction in aqueous solution: 5Br−(??) + BrO3−(??) + 6H+(??) ⟶…

Q: The kinetics of a particular reaction are described by the following rate law: Rate = k (A][B]*[C]…

A: The kinetics of the considered reaction has been described by the rate law as,

Q: An experiment produced the data presented in the following Table. What is the instantaneous rate of…

A: The rate of the reaction refers to the speed at which the reactant gets converted to product. The…

Q: 3A+B+C → D+Ewhere the rate law is defined as_ Δ|A|/Δr = k[A]2 [B] [C]An experiment is carried out…

Q: The reaction is first order in N2O5. For this reaction at 45oC, the rate constant k = 1.0 × 10–5…

Q: What is the concentration of a reactant after 20.5 s

Q: L00524 M-1. s-1. missing entries in the table? [C,H,Br, ]o (M) [lo (M) Initial rate of formation of…

A: x = 0.7799M y = 0.3905M z = 0.000199Ms-1

Q: The rate law for the reaction of NO2(g) with CO(g) to produce NO(g) and CO2(g) is second order in…

Q: The reaction between nitrogen dioxide and carbon monoxide is NO₂(g) + CO(g) → NO(g) + CO₂(g) The…

Q: Given the following data taken at 300 K, determine the rate law for the reaction: 2 NO(g) + Cl2(g)…

A: For a given reaction - 2 NO + Cl2 ---> 2 NOCl Rate law will be expressed as Rate = k [NO]x…

Q: Consider a reaction: A + B-→ C and the rate law expression: Rate = k [A]"[B]" %3D

Q: The rate law for the general reaction: aA + bB → cC + dD is rate = k[A]α[B]β…

A: Given aA + bB → cC + dD rate = k[A]α[B]β

Q: 1. Nitrogen monoxide, NO, reacts with hydrogen to give nitrous oxide, N₂O2, and water, as…

Q: For the decomposition of gaseous dinitrogen pentoxide, 2N₂O₅(g) → 4NO₂(g) + O₂(g) the rate constant…

A: The objective of the question is to calculate the mole fraction of .

Q: The rate law for a reaction is determined to be rate=k[X]3[Y]. What is the overall order of this…

Q: Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A] where k=2.90 ×10-4…

A: Given, k=2.90 ×10-4 s-1 [A] = 0.0500 M

Q: The experimentally determined rate law for the reaction: 2N2O5(g) ® 4NO2(g) + O2(g) is Rate…

A: The rate law of a reaction is the theoretical approach in determining the relation between the rate…

Q: w long

Q: С,Н, Вr, (aq) + 3Г(аq) — C,H,(g) + 2 Br¯(aq) + I5 (aq) ne rate law is k[C,H¸B1, ][I¯] rate = nere k…

Q: Consider a reaction: A + B C and the rate law expression: Rate = k [A]"'[B]" If the reaction is zero…

A: Given: A+B→C Rate law: Rate=kAmBn Order of A=0 Order of B=1 To find: Values of m and n Solution :…

Q: The rate of the reaction 2 CIO2(aq) + 2 OH" (aq) → ClO, (aq) + ClO (aq) + H2O(€) is given by rate =…

A: The rate law of the reaction is given as, => Rate = K [ClO2]2 [OH- ] Given: Initial concentration…

Q: How to use calculus to integrate the differential rate law and obtain the first-order integrated…

A: The given first-order integrated rate law is,

Q: Consider this reaction: 2C1₂05 (g) → 2Cl₂(g) +50₂ (g) - At a certain temperature it obeys this rate…

A: The formula used is:- Kt = 2.303 log [A]o [ A]t K = rate constant t =time [A]o = initial…

Q: Consider a reaction: A + B C and the rate law expression: Rate = k [AJ"[BJ' If the reaction is zero…

A: A+B → C RATE = K [A]m [B]n where m = order of reaction with respect to concentration A n…

Q: For a reaction that obeys the rate law: rate = k[A]°[B]² %3D The order of this reaction with respect…

A: Explanation to the correct answer is given below

Q: What are the units of k in the following rate law? Rate = k[X]0 [Y]0 Ms 1/s s/M2 M/s M-1s-1

A: Given, the rate law: Rate = k[X]0 [Y]0 We have to find the unit of k.

Q: Determine the molecularity of the reaction given the following rate law: Rate = k[A]2

A: Rate = k[A]2

Q: O3(g)→O2(g)+O(g) Using the results of the Arrhenius analysis (Ea=93.1kJ/molEa=93.1kJ/mol and…

A: All the data is given in question Formula to be used is K=Ae-EaRT A= pre-exponential factor Ea=…

Q: Cyclopropane, C3H6, is converted to its isomer propylene, CH₂=CHCH3, when heated. The rate law is…

A: As the given reaction follows first order rate kinetics, the rate constant can be expressed as:…

Q: Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A]2 where k=2.90 ×10-2…

A: For the given reaction, Rate law has been defined as : Rate = k [A]2 From…

Q: Consider the following reaction in aqueous solution: 5Br−(??) + BrO3−(??) + 6H+(??) ⟶…

Q: The reaction A + 2B → C proceeds according to the rate law, rate = k[A][B] with k = 8.50 x 10-3 M-1…

A: For a reaction , A + B = C The rate of the reaction will be, R = K [A][B] Where K is the rate…

Q: temperature it obeys this rate law. ate = = (0.0317 M¹-¹) [₂05] S se a vessel contains N₂O5 at a…

Question

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: to determine

VIEW

Step 2: determination of the value of k

VIEW

Solution

VIEW

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider this reaction: CICH,CH,CI (g) → CH,CHCI (g) +HCI (g) At a certain temperature it obeys this rate law. rate = (0.00421 s*)[CICH,CH,CI] S Suppose a vessel contains CICH,CH,Cl at a concentration of 1.13 M. Calculate how long it takes for the concentration of CICH,CH,Cl to decrease by 85.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. ?
Consider the mechanism. Step 1: 2A — В +С slow Step 2: В +С — Е fast Overall: 2А — Е Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =
Consider the following proposed mechanism for the reaction: 2 NO2Cl (g) → 2 NO2 (g) + Cl2 (g) step 1 (slow): NO2Cl (g) → NO2 (g) + Cl (g) step 2 (fast): Cl (g) + NO2Cl (g) → NO2 (g) + Cl2 (g) What is the rate law consistent with this mechanism? rate = k[NO2][Cl2] rate = k[NO2Cl] rate = k[NO2Cl]2 rate = k[NO2Cl]2[Cl] rate = k[NO2Cl][Cl please answer ASAP
Consider the rate law: Rate = k [A]2[B][C]1/2. How does the rate of the reaction change if the concentration of C is doubled? The rate increases by a factor of 1.414 The rate increases by a factor of 1.732 The rate reduces by a factor of 1.732 The rate triples The rate reduces by a factor of 1.414
The reaction A → B + C is known to be zero order in A with a rate constant of 5.2 × 10–2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 3.2 × 10–3 M. What is the half-life for the reaction? A) 1.3× 101 s B) 2.6× 10–2 s C) 8.3× 10–2 s D) 6.0× 104 s E) 3.1× 10–2 s
Consider the mechanism. Step 1: 2 A = B + C equilibrium Step 2: В +D — E slow Overall: 2A + D — С +Е Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) +O₂ (g) At a certain temperature it obeys this rate law. rate = (0.0328 s−¹)[N₂05] S Suppose a vessel contains N₂O5 at a concentration of 0.860M. Calculate the concentration of N₂O5 in the vessel 22.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
Consider the reaction aA + bB dD + eE C = catalyst The rate law is Rate = k[A]ª[B][C]S Which of the following statements is incorrect? The exponents q and r are always equal to the coefficients a and b, respectively. The overall reaction order is q + r+ s. O The exponent s must be determined experimentally. The symbol k represents the rate constant. O The exponents q, r, and s are often integers.
Consider the reaction, A + B + C => D, which is found to be first order in A, first order in B and first order in C. Which step of the proposed mechanism must be slow in order to agree with this rate law? 1. A(g) + B(g) => X(g) 2. X(g) + C(g) => Y(g) 3. Y(g) => D(g) A. 1 B. only 3 C. Either 2 or 3 D. only 2
Consider following reaction: 2 A2B5(g) → 4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;
The isomerization of cyclopropane, C3H6, is believed to occur by the mechanism shown in the equations above. Here C3H6* is an excited cyclopropane molecule. At low pressure, Step 1 is much slower than Step 2. Derive the rate law for this mechanism at low pressure?
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T