Consider a hypothetical reaction: A→ 3B + C The reaction is 2nd order and k = 0.0220 M-¹s-¹. Starting with initial [A] = 0.195 M and no other substance in the container, calculate [B] after 24.0 seconds of reaction time. Hint: Solve for final concentration of A and use stoichiometry.

Consider a hypothetical reaction: A→ 3B + C The reaction is 2nd order and k = 0.0220 M-¹s-¹. Starting with initial [A] = 0.195 M and no other substance in the container, calculate [B] after 24.0 seconds of reaction time. Hint: Solve for final concentration of A and use stoichiometry.

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: 2) The following reaction occurs at 200 K: A + B + C → X Based on the tabulated data from…

A: The speed of the reaction is measured in terms of rate of reaction. The rate of reaction is defined…

Q: Calculate the rate constant, K at 904 °C.

Q: how do i determine if the reaction 2HI(g) ---> H2(g) + I2(g) is first order or second order based on…

A: The order of reaction is to be determined.

Q: 5. The reaction A → B+C is known to be first order in A. Below are data showing the concentration of…

A: Given is a first order reaction.To find the average rate, instantaneous rate and rate constant for…

Q: Consider the hypothetical reaction A(g) + B(g) ---> C(g) The four containers below…

A: In the given image, the number of atoms of A and B present in container X is 2 and 4, respectively.…

Q: 1. The reaction, 2A + B → C, is studied by monitoring the concentration of A. Over the first 3.2…

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

Q: 17. Consider the zero-order reaction A → Products, with a rate constant k = 4.0 X 10-3 M s 1. If…

Q: Question 13: The decomposition of hydrogen peroxide: H202 -> H2 + 02 is a first order reaction with…

A: Answer:Since, decomposition reaction of H2 is first order, therefore

Q: A certain reaction is first order in H, and first order in I. Use this information to complete the…

A: Given: The reaction is first-order in both H2 and I2. And the data given is,

Q: The reaction 2NO (g) +0_2(g)>2NO_2 (g) has the following rate law: K[0_2][NO]^2. if the…

A: assuming initial [O2] = x and [NO] = y Hence the Rate = K[O2][NO]2 = Kxy2 Now new concentrations are…

Q: The kinetics of the reaction 3 A → B was studied by monitoring the concentration of A as a function…

A: Given a graph of reaction 3A ----> B

Q: For a starting concentration of 1.0 M, the concentration after 5 minutes for a first-order reaction…

A: For a first order reaction the rate law can be written as, rate= k[A] Where [A] is the…

Q: A certain reaction is second order in N, and first order in H,. Use this information to complete the…

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

Q: A chemistry graduate student is studying the rate of this reaction: 2H3PO4 (aq) → P₂O5 (aq) + 3H₂O…

A: The given reaction is:Let us consider the second-order rate of reaction..

Q: A student plots their concentration and time data from a lab they performed to determine the order…

A: Order of reaction: according to chemical kinetics order of reaction is define as the power…

Q: The reaction 2A + 3B -> C is first order with respect to A and B. When the initial concentrations…

A: The specific rate constant or rate constant (k) is the proportionality constant relating the rate of…

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: Which of the following plots is consistent with a zero-order reaction?

A: The speed at which a chemical reaction takes place is known as the rate of the reaction. It is…

Q: Consider the reaction data. A⟶products ? (?) ? (?−1) 325 0.391 575 0.735 What two points…

Q: What is the reaction order? Calculate the concentration of A after 129 s. [A]129 s = M

Q: A certain reaction is first order in H, and first order in I,. Use this information to complete the…

A: Rate of reaction The decrease of concentration of reactants per unit time or increase of products…

Q: A certain reaction is first order in H, and first order in I₂. Use this information to complete the…

Q: 4. For the reaction M,X>2 M+X the following data was recorded: Time (h) [M-X] (М) 0.00 0.100 1.00…

A: From the given data, plots are drawn as shown below. From the regression line, the more close to 1,…

Q: A certain reaction is first order in H, and first order in I,. Use this information to complete the…

A: a Rate of raection=kH2 I2 where k is rate constant2×105 ms-1 =k1.45m 1.44mRate of reaction=kH2 I2…

Q: 81. The following data were obtained for the reaction 2A + B →C where rate = d{A]/dt %3D [A](M)…

A: The rate of a reaction is directly proportional to the concentration of reactant raise to the power…

Q: Be sure to answer all parts. For the reaction 4A(g) + 3B(g) →→→ 2C(g) The following data were…

A: Determine the reaction order with respect to each reactant based on data.

Q: A certain reaction is first order in H, and first order in I,. Use this information to complete the…

Q: 2. For the following reaction at 500 °C Cl2 (g) H2 (g) + 2 HCI (g) the following data were…

Q: NO2(e) + CO(g) NO(g) + CO2(g) Rate (M/sec) Initial [NO2] Initial [CO ] 1.1 x 10-2 0.15 0.1 4.5 x…

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

A: Given: [A] (M) t (s) Ln[A] 1/[A] 0.750 0.0 -0.2877 1.334 0.596 30.0…

Question

100%

Consider a hypothetical reaction: A → 3B + C
The reaction is 2nd order and k = 0.0220 M-¹s-¹.
Starting with initial [A] = 0.195 M and no other substance in the container, calculate [B] after 24.0 seconds of reaction time.
Hint: Solve for final concentration of A and use stoichiometry.

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: Rate constant for second order reaction

VIEW

Step 2: Concentration of A after 24.0 second

VIEW

Step 3: Concentration of B after 24.0 s

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 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

A chemistry graduate student is studying the rate of this reaction: 2C1,0, (g)- 2C1, (g) +50, (g) He fills a reaction vessel with Cl,0, and measures its concentration as the reaction proceeds: time [C,0,] (seconds) 0| 0.0900 M 10. 0.0579 M 20. 0.0372 M 30. 0.0239 M 40. 0.0154 M Use this data to answer the following questions. Write the rate law for this reaction. rate Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
A certain reaction is second order in N, and first order in H₂. Use this information to complete the table below. Round each of your answers to 3 significant digits. [₂] 1.94 M 1.94 M 3.73 M 1.34 M 6.33 M 0.697 M initial rate of reaction 0.349 M/s M/S M/S X
n
The rate of a certain reaction is given by the following rate law: rate =k N, O, Use this information to answer the questions below. olo What is the reaction order in N,? |x10 18 Ar What is the reaction order in 03? What is overall reaction order? At a certain concentration of N, and 03, the initial rate of reaction is 0.780 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 103M/s when [N2] = 1.1 M and [03] = 1.1 M. Calculate the value of - 3 -1 k = |M •S the rate constant. Round your answer to 2 significant digits.
6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179
Consider the reaction I- + OCl- → OH-→ IO- + Cl- Determine the reaction's rate law using the given experimental data. Exp # [I-]o [OCl-]o [OH-]o Initial Rate (M/s) 1 0.0013 0.012 0.10 0.094 2 0.0026 0.012 0.10 0.187 3 0.0013 0.006 0.10 0.047 4 0.0013 0.012 0.20 0.047
What amount of time is required for the concentration of A to decrease from 0.800 M to 0.180 M in the zero- order reaction A->B? (k = 0.0567 M*s1)
1. Given the following data, determine the orders (m and n) with respect to the concentrations of A and B in the reaction Orders: [A] 0.020 M 0.020 M 0.010 M 0.010 M m= A+B products Rate = k[A][B]" [B] 0.020 M 0.010 M 0.020 M 0.010 M n = Time for reaction 19 sec 19 sec 76 sec 76 sec What time would you predict if both concentrations of A and B were made to be 0.040 M?
A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [4.] initial rate of reaction x10 1.91 M 0.885 M 0.894 M/s olo 0.813 M 0.885 M I|| M/s Ar 0.213 M 7.92 M
The reaction A →B is found to be first order. At 650 K, 45 % of A has been converted to B in 75.0 minutes. At 650 K, calculate the rate constant of this reaction with the unit s O A. 1.77 x 1045-1 O B. 3.59 x 102 s-1 O. 2.72 x 10-6 5-1 O D. 1.33 x 1045-1 E. 1.82 x 10-6 5-1
Please provide expl
A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. initial rate of reaction x10 0.537 M 0.350 M 21.0 M/s 0.169 M 0.350 M || M/s 0.261 M 0.721 M M/s