koth 3.33x10-4 MSubmit Previous AnswersCorrectPart B[A]o = 3.25. 10SubmitWhat was the initial reactant concentration for the reaction described in Part A?Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.► View Available Hint(s)for Rart B for Part B do for Part redo for eart B resor Part B keyboard shortcuts for Part B help for Part BPart CX Incorrect; Try Again; 5 attempts remaining-2Previous Answers2kist= 3.26 107Part DSubmit Previous Answersk2nd =MThe reactant concentration in a first-order reaction was 8.20x10-2 Mafter 30.0 s and 8.40x10-3 M after 100 s. What is the rate constant for this reaction?Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.► View Available Hint(s)SubmitSfor Rart C for Part Cdo fdo for Part redo for eart C resor Part C keyboard shortcuts for Part C help for Part CX Incorrect; Try Again; 4 attempts remainingValueMSThe reactant concentration in a second-order reaction was 0.350 Mafter 185 s and 1.50x10-2 Mafter 785 s. What is the rate constant for this reaction?Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.► View Available Hint(s)for Part D for Part Ddo fo}do for Parti0Units3redo for eart D resor Part D keyboard shortcuts for Part D help for Part D The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line,y=mx+b.Order012Integrated Rate Law[A] = - kt + [A]o| In[A] = −kt + ln[A]oA= kt+1[A]oGraph[A] vs. tSlope-kIn[A] vs. t -kkAvs. t

Please note that Part B is an Incomplete Question. To solve the same Part A (or complete…

The reactant concentration in a first-order reaction was 8.20x10-2 Mafter 30.0 s and 8.40x10-3 M after 100s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. ▸View Available Hint(s) for Rart C for Part Cdo for Part redo for eart C restor Part C keyboard shortcuts for Part C help for Part C M kist 3.26 10 Submit Previous Answers S X Incorrect; Try Again; 4 attempts remaining Part D The reactant concentration in a second-order reaction was 0.350 M after 185 s and 1.50x10-2 M after 785 s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.

The reactant concentration in a first-order reaction was 8.20x10-2 Mafter 30.0 s and 8.40x10-3 M after 100s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. ▸View Available Hint(s) for Rart C for Part Cdo for Part redo for eart C restor Part C keyboard shortcuts for Part C help for Part C M kist 3.26 10 Submit Previous Answers S X Incorrect; Try Again; 4 attempts remaining Part D The reactant concentration in a second-order reaction was 0.350 M after 185 s and 1.50x10-2 M after 785 s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.7: Reaction Mechanisms

Problem 11.12E

See similar textbooks

Related questions

Q: 5) The homogeneous reaction in aqueous solution DO NOT USE STEADY STATE IO3 + 81 + 6H→ 313 + 3H₂0…

A: The objective of this question is to determine the rate law for the given equations.

Q: For A → products, time and concentration data were collected and plotted as shown. [A] (M) t (s)…

A: According to the graphical method of finding the order of the reaction If the graph of…

Q: 2NO + O2 = 2NO2 The rate law is –D[NO]/Dt = k[NO]2[O2], where k is 1.16x10-5 L2/(mol2 s) at…

Q: access important values if needed for this question. The reaction of nitrogen dioxide with fluorine…

Q: 20For the generic reaction 2A=> C + 2D it was determined that teach half-life of the reaction is the…

Q: The reactant concentration in a first-order reaction was 6.50x10-2 M after 50.0 s and 6.10x10-3 M…

Q: A mechanism for the gas prase step 1 slow: F₂ + CIO2 → FCIO2 + F step 2 fast: F + CIO₂ →→ FCIO2 (1)…

A: The given two steps of the reaction are: Step 1: F2+ClO2→FClO2+F slowStep 2: F+ClO2→FClO2 fast For a…

Q: For A products, time and concentration data were collected and plotted as shown. 1 [A] (M) t(s)…

A: The reaction order is determined by the relationship between the rate of reaction and the…

Q: A) Determine the order with respects to H2 and the order with respect to O2. Explain reasoning. B)…

Q: ± Half-life (kinetics) for First Order Reactions I Review | Constants | Periodic Table Half-life…

A: Rate constant = 7.40 x 10-4 s-1 Order of reaction = 1

Q: will it take for the reactant concentration

A: Part-B : You can used direactly half life equation for first order reaction, Rate constant =…

Q: Determine the rate constant (with appropriate unit) and reaction orders of the reaction of A + B à C…

A: First write down the rate law for each trial and then taking ratios, find out the rate constant and…

Q: P) For a particular first-order reaction, it takes 48 minutes for the concentration of the reactant…

Q: For the reaction: A (g) + B(g) the rate is 0.27 [B] =3.7 mol L's - mol L.s AB (g) when [A], [B], 1.0…

A: First order in B and second order in A.rate law is M =

Q: For the reaction A (g) + B (g) + C (g) → D (g) the following data were obtained at constant…

A: The given reaction is: A (g) +B (g) +C(g) →D(g)Let the rate law be:6.25×10-3 =k(0.05)a (0.05)b…

Q: Consider the second-order reaction: 2HI(g)→H₂(g) + I2(g) Use the simulation to find the initial…

A: We have the second order reaction :We need to find the concentration of HI after the given time.We…

Q: 4.) Nitric oxide reacts with hydrogen at 1280 °C according to the reaction below. Using the…

A: The overall order of the reaction can be described as the addition of the mathematical exponent…

Q: 2. Decomposition k (S¹) T (°C) of an organic compound is a first-order reaction. Consider the data:…

A: Given is a table of values of rate constant (k) at different temperatures(T) of a first-order…

Q: The following reaction is first order in respect to CH3OH and first order in respect to HCl. With…

A: First-order reaction:The rate of the first-order reaction depends only on one reactant. The given…

Q: Calculate the value of the rate constant k. Round to two sig figs. Use the right unit system as well…

A: Rate law:The given reaction is,

Question

koth 3.33x10-4 M
Submit Previous Answers
Correct
Part B
[A]o = 3.25. 10
Submit
What was the initial reactant concentration for the reaction described in Part A?
Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
► View Available Hint(s)
for Rart B for Part B do for Part redo for eart B resor Part B keyboard shortcuts for Part B help for Part B
Part C
X Incorrect; Try Again; 5 attempts remaining
-2
Previous Answers
2
kist= 3.26 107
Part D
Submit Previous Answers
k2nd =
M
The reactant concentration in a first-order reaction was 8.20x10-2 Mafter 30.0 s and 8.40x10-3 M after 100 s. What is the rate constant for this reaction?
Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
► View Available Hint(s)
Submit
S
for Rart C for Part Cdo f
do for Part redo for eart C resor Part C keyboard shortcuts for Part C help for Part C
X Incorrect; Try Again; 4 attempts remaining
Value
M
S
The reactant concentration in a second-order reaction was 0.350 Mafter 185 s and 1.50x10-2 Mafter 785 s. What is the rate constant for this reaction?
Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
► View Available Hint(s)
for Part D for Part Ddo fo
}
do for Parti
0
Units
3
redo for eart D resor Part D keyboard shortcuts for Part D help for Part D

The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line,
y=mx+b.
Order
0
1
2
Integrated Rate Law
[A] = - kt + [A]o
| In[A] = −kt + ln[A]o
A
= kt+
1
[A]o
Graph
[A] vs. t
Slope
-k
In[A] vs. t -k
k
A
vs. t

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Introduction.

VIEW

Step 2: Calculating Rate constant for Part C.

VIEW

Step 3: Calculating Rate constant for Part C Contd...

VIEW

Step 4: Calculating Rate constant for Part D.

VIEW

Step 5: Calculating Rate constant for Part D Contd...

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 6 steps

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

The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
The decomposition of azomethane, (CH3)2N2, to nitrogen and ethane gases is a first-order reaction, (CH3)2N2(g)N2(g)+C2H6(g). At a certain temperature, a 29-mg sample of azomethane is reduced to 12 mg in 1.4 s. (a) What is the rate constant k for the decomposition at that temperature? (b) What is the half-life of the decomposition? (c) How long will it take to decompose 78% of the azomethane?
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
If you know some calculus, derive the integrated first-order rate law for the reaction by following these steps: Define the reaction rate in terms of [A]. Write the rate law in terms of [A], k, and t. Separate variables in the rate law. Integrate the rate law. Write the integrated equation in the form . Derive the half-life as was done in Section 11-3c.
Hundreds of different reactions occur in the stratosphere, among them reactions that destroy the Earths ozone layer. The table below lists several (second-order) reactions of Cl atoms with ozone and organic compounds; each is given with its rate constant. For equal concentrations of Cl and the other reactant, which is the slowest reaction? Which is the fastest reaction?
One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?
Many biochemical reactions are catalyzed by acids. A typical mechanism consistent with the experimental results (in which HA is the acid and X is the reactant) is Step 1: Step 2: Step 3: Derive the rate law from this mechanism. Determine the order of reaction with respect to HA. Determine how doubling the concentration of HA would affect the rate of the reaction.