Based on the following data for thefırst order reaction Jproducts, calculatethe rate constant k (in s1).Time[J]Os1.0000 M900.52313000.1153O 2.9 x 104O 1.4 x 103O 5.3 x 10-4О 1.0 х 10-3O 7.2 x 10-4 R = .008314 kJ/K (Gas Constant)F = 96.485 kJ/(V mol)[A]pK, + log(班)[base]pHpK, + logORpH%3D[acid][HA]AG°AH° - TASºAG = AG° + RTINQAG° = -RT/nKeqAG° = -nFE°cell%3D0591EcellE°clllogQFirst OrderRadioactivitySecond Order[AloInXo1ktIn= kt= kt +[A]t[A][A]o.693.693ty =ty =ty =kkK[A]

We will use intergrated rate law for first order reaction to calculate rate constant.

Based on the following data for the fırst order reaction J products, calculate the rate constant k (in s-1). Time [J] Os 1.0000 M 900 .5231 3000 .1153 O 2.9 x 10-4 Ο 1.4 x 103 O 5.3 x 10-4 O 1.0 x 10-3 O 7.2 x 10-4

Based on the following data for the fırst order reaction J products, calculate the rate constant k (in s-1). Time [J] Os 1.0000 M 900 .5231 3000 .1153 O 2.9 x 10-4 Ο 1.4 x 103 O 5.3 x 10-4 O 1.0 x 10-3 O 7.2 x 10-4

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: How long will it take for the concentration of A to decrease from 1.400 M to 0.205 for the zero…

Q: How long will it take for the concentration of A to decrease from 1.25 M to 0.357 for the second…

Q: The rate constant for the reactionBr(g)+O3(g) -> BrO(g)+O2(g)was determined at the four…

A: The Arrhenius equation that gives the relation between rate constant (k), temperature (T), and…

Q: reaction of a particular organic compound with water varies with temperature as follows:…

Q: Given the following rate constants: K1= 5.2x10-10 M-1s-1 at 300. K ; K2=7.3x10-9M-1s-1 at 320. K…

A: Solution to calculate Ea :-

Q: 13. Consider the following data: #drinks 1 2 24 4 [C₂H,OH ] (M) Rate (M/h) 0.055 2.0 × 10-2 0.110…

A: 1.Order is the sum of the power of reactant concentration in rate law expression. 2. Rate constant…

Q: a. What are the orders of reaction with respect to each reactant, and what is the overall order of…

Q: Using the following rate law and the experimental values, calculate k for each experiment and…

Q: How long will it take for the concentration of A to decrease from 1.25 M to 0.299 for the second…

Q: for a given first order reaction after 3.00 min 5.0% of the reactsnt remains. calculate the rate…

A: Rate law: According to the rate law, the rate of a reaction is directly proportional to the product…

Q: What is the activation energy for a reaction if the rate constant is 1.75 × 10 -4 s -1 at 220°C K…

Q: The following reaction has a rate constant of 0.760s-1 at 1000. K and a rate constant of 0.870s-1 at…

Q: 2. The following data were collected for the reaction between hydrogen and nitric oxide at 700 °C:…

A: 2.Rate of a reaction is proportional to the molar concentration of reactants raised to some powers…

Q: How long will it take for the concentration of A to decrease from 1.25 M to 0.249 for the second…

Q: Use the following table of initial rate data to determine the orders of reactants A and B in the…

Q: The rate constant for the reactionBr(g)+O3(g)---->BrO(g)+O2(g)was determined at the four…

A: To plot the graph the values of 1/T and ln k is determined.

Q: 16. The rate constant for a second order reaction R→ products is 2.60 x 102 M¹s¹. How many seconds…

Q: How long will it take for the concentration of A to decrease from 1.25 M to 0.205 for the second…

A: The time taken has to be calculated.

Q: How long will it take for the concentration of A to decrease from 1.400 M to 0.275 for the zero…

A: The initial concentration of A is .The final concentration of A is .The rate constant of the…

Q: The rate constant of a certain reaction is 7.3 × 10-4 s-1 at 300 K. If the activation energy is 45.1…

A: Step 1: State the given: Initial rate constant, k1 = 7.3 x 10-4 s-1Activation energy, Ea = 45.1…

Q: For the decomposition of the acceptor---nitrate complex: acceptor•NO3 - acceptor + NO3 the rate…

A: For the decomposition of the acceptor---nitrate complex: acceptor .NO3- ----> acceptor + NO3-…

Q: The rate of a reaction A + 2B products is determined. When the concentration of A is 1.0 M, the rate…

A: Rate law gives the relationship between the rate and concentration of the reactants. Rate = k[A]n…

Q: Using the Arrhenius equation to calculate k at one temperatur... The rate constant of a certain…

Q: The following data were measured for the reaction OCl-(aq) + I-(aq) ---> OI-(aq) + Cl-(aq)…

Q: 3. The following rate constants were measured for a particular reaction: ki = 2.5 x 101 s' at 300. K…

Q: The reaction 2A--->P has a rate constant k= 3.50 x 10-4 dm6 mol-2s-1 What is the order of this…

A: For reaction, 2A----> P Rate constant (k) = 3.50 ×10-4 dm6 mol-2s-1 Order of reaction = ?

Q: How long will it take for the concentration of A to decrease from 1.25 M to 0.229 for the second…

A: Initial concentration of A = 1.25 M Reduced concentration of A = 0.269 M Rate constant (k) = 1.52…

Q: Determine the rate law and the value of k for the following reaction using the data provided:…

Q: How long will it take for the concentration of A to decrease from 1.400 M to 0.245 for the zero…

A: Provided initial concentration [A•]= 1.400M Provided final concentration [A]=0.245M Rate constant…

Q: Consider the following elementary reaction: NO2(g)+F2(g)→NO2F(g)+F(g) Suppose we let k1 stand for…

Q: The reaction rate for the decomposition of N2O5 to form NO2 and O2 was studied as a function of…

Q: The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an…

Q: How long will it take for the concentration of A to decrease from 1.25 M to 0.269 for the second…

A: Initial concentration of A = 1.25 M Reduced concentration of A = 0.269 M Rate constant (k) = 1.52…

Q: EX7 The first-order bidirectional reaction is given: k₁ k.1 with rate constantsk₁=5 x 10-²S-¹ and…

Q: At a given temperature, the elementary reaction A↽−−⇀B,A↽−−⇀B, in the forward direction, is first…

Q: Consider the reaction 2HI→ H₂+I2. The rate of disappearance of HI follows the second order rate law.…

Q: Consider the elementary reactions and their rate constants. kg = 4.99 × 10-2 k, = 3.67 × 10-1s-1…

Q: What is the value of the equilibrium constant for the reaction A B at this temper

A: As we know, A) Equilibrium constant (K) = Kf/Kb = 0.0230/0.0590 K = 0.390

Q: At a given temperature, the elementary reaction A↽−−⇀B, in the forward direction, is first order in…

A: for an elementary reaction, A⇔B the forward rate constant, Kf = 0.0270 s-1 the reverse reaction rate…

Q: Determine the rate law and the value of k for the following reaction using the data provided. 2…

A: Recall the given reaction,…

Q: At a given temperature, the elementary reaction A = B, in the forward direction, is first order in A…

A: The brief calculation of equilibrium constant for both the reaction is given below

Q: The rate constant for the reactionBr(g)+O3(g) --> BrO(g)+O2(g)was determined at the four…

A: The Arrhenius equation that gives the relation between rate constant (k), temperature (T), and…

Q: Nitrogen diaxide is a highly reactive gas! Determine the rate law and the value of k for the…

Q: @33 °C Cr(H₂O)6³ +SCN ---> Cr(H₂O)5NCS² + H₂O(1) Initial Rate 2.0x10-¹1 2.0x10-10 9.0x10-10 2.4x10-⁹…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Q: NO,(0) + O3(g) → NO3(g) + O,(g) [NO2li (M) 0.1 0.1 Initial Rate (ms1) [O3li (M) 0.33 1 1.42 2 0.66…

Question

100%

Based on the following data for the
fırst order reaction J
products, calculate
the rate constant k (in s1).
Time
[J]
Os
1.0000 M
900
.5231
3000
.1153
O 2.9 x 104
O 1.4 x 103
O 5.3 x 10-4
О 1.0 х 10-3
O 7.2 x 10-4

R = .008314 kJ/K (Gas Constant)
F = 96.485 kJ/(V mol)
[A]
pK, + log
(班)
[base]
pH
pK, + log
OR
pH
%3D
[acid]
[HA]
AG°
AH° - TASº
AG = AG° + RTINQ
AG° = -RT/nKeq
AG° = -nFE°cell
%3D
0591
Ecell
E°cll
logQ
First Order
Radioactivity
Second Order
[Alo
In
Xo
1
kt
In
= kt
= kt +
[A]t
[A]
[A]o
.693
.693
ty =
ty =
ty =
k
k
K[A]

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 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

For the interconversion between A and B as shown below, which of the following describes how the equilibrium constant (K) is related to the rate constants k1 and k -1 and to the amounts of A and B present at equilibrium? k1 A В k.1 OK = kj[A] and K = kj[B] k[B] K = kj[A] [B] K and K || [A] k1 [B] [A] K and K %3D k-1 k[A] K = kj[B]
Consider the following elementary reaction: H,(9) +2NO(g) → N,0(g) +H,O(g) Suppose we let k, stand for the rate constant of this reaction, and k_, stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of H,O in terms of k, k_1, and the equilibrium concentrations of H, NO, and N,O. [H,0]= 0 %3D
Determine the rate law and calculate the rate constant for this reaction: 2 NO (g) + Br₂(1)→2 NOBr (g) Initial [Br₂]/M Expt. 1 2 3 Initial [NO]/M 0.10 0.20 0.20 0.10 0.10 0.30 Initial rate/M.s-¹ 1.30 x 10-³ 5.20 x 10-³ 1.56 x 10-²
The reaction 2A--->P has a rate constant k= 3.50 x 10-4 dm6 mol-2s-1What is the order of this reaction? Why?
The rate law for a given reaction is rate = k[reactant]?, with k = 2.64 x 10-4 M-1 min 1. If the initial concentration is 0.0250 M, what is the initial rate, with the correct units? A 4.36 x 10 11 M min 1 1.65 x 107 min 1 C 6.60 x 10-6 M min 1 1.65 x 10-7 M min 1 O A O B O C OD Next « Previous
The values of the rate constant for the A→Products reaction are given in the table below with the change of temperature. Find the activation energy for this reaction. k 0.027 0.040 0.059 0.085 0.12 0.17 0.24 t (oC) 1 6 11 16 21 26 31
If the order of the reaction is first order for both reagents then using the rate law and the following data solve for K. Rate 1.9 X 10^-6 [I-] = 0.45 M [H2O2] = 0.125 M O A. 1.1 X 10^-5 O B.3.4 X 10^-5 O C. 3.4 X 10^-4 O D. 1.1 X 10^-7
How long will it take for the concentration of A to decrease from 1.25 M to 0.253 for the second order reaction A → Products? (k = 1.52 M¹min¹)
A reaction A - products has a constant rate. The concentration of A starts at 1.00 M. If the rate constant is 0.0015 M s-1, what is the concentration of [A] after 3 minutes? 0.787 M 0.730 M O 0.763 M O 0.270 M O 0.996 M
How long will it take for the concentration of A to decrease from 1.400 M to 0.555 for the zero order reaction A → Products? (k = 0.0345 M/s)
r = L [A] [B] ² x2 x 2 r=k [2A) [21] ² 8x bigger than 2 + 4 = 8 12. Consider a reaction of the form 2A + BC. The data for this reaction is given below: Initial rate of formation of C M/s Initial [A] Initial [B] 4.0 x 10-² 0.30 0.10 2.0 x 10-² 0.50 0.05 6.0 x 10-² 0.50 0.15 1.0 x 10-² 0.025 a. What rate law is consistent with this data? 0.40 b. Calculate k and specify units. How long will it take for the concentration of C to equal to 0.10 molar if the initial concentration of all the species are [A] = 0.4 M, [B] = 0.3 M and [C] = 0.0 M?
Determine the rate law and the value of k for the following reaction using the data provided. S20g2 (aq) + 3 1'(aq) → 2 SO4² (g) + [S20g2]; (M)[I"]; (M) Initial Rate (M/s) 13 (aq) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33 O Rate = [86 M-2s 1[S20g2-1[17? %3D O Rate = [195 M-3s-1[S20g²1²{u]² %3D O Rate = [23 M-1/25-1][S20g²-][1]1/2 %3D O Rate = [36 M-15-1|[S20g² 1[1'] %3D O Rate = [120 M-2s-1][S20g2-1²{1'] %3D