Some measurements of the initial rate of a certain reaction are given in the table below. [N] [H.] initial rate of reaction 1.21M 2.36M 5.00 × 10*M/s 1.21M| 0.916М 7.53 × 10°M/s 2.08M| 2.36M 8.60 x 10*M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k |I| k =

Some measurements of the initial rate of a certain reaction are given in the table below. [N] [H.] initial rate of reaction 1.21M 2.36M 5.00 × 10M/s 1.21M| 0.916М 7.53 × 10°M/s 2.08M| 2.36M 8.60 x 10M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k |I| k =

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter16: Reaction Rates

Section: Chapter Questions

Problem 6STP

See similar textbooks

Related questions

Q: Some measurements of the initial rate of a certain reaction are given in the table below. N2|H2|…

Q: Some measurements of the initial rate of a certain reaction are given in the table below. [N:]…

Q: Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2…

Q: A chemistry graduate student is studying the rate of this reaction: →H2CO3aq+H2OaqCO2aq She fills a…

Q: Calculate the concentration of NH4OH in the vessel 0.150 seconds later.

Q: Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂]…

Q: A chemistry graduate student is studying the rate of this reaction: 2NH₂(g) → N₂ (g) + 3H₂(g) She…

A: Answer: This question is based on trial and error method where we will put the given data in the…

Q: Some measurements of the initial rate of a certain reaction are given in the table below. [H.] 12…

A: Given: [H2] [I2] RATE 1.78 M 0.743 M 0.666 M/s 0.879 M 0.743 M 0.329 M/s 1.78 M 2.67 M 2.39…

Q: Concentration and rate data are provided in the table below for the reaction shown. 2NO(g) + Cl,(g)…

A: First find the orders with respect to NO and Cl2 then find k . Put these values in data 4 to find…

Q: Given the information below, determine the rate law for the reaction and the rate constant (k). Be…

A: Rate law: K[A]2[B]1 Rate constant K = 1.5 M-2s-1

Q: Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂]…

A: Suppose the rate law expression for the reaction is: Rate = k * [N2]X * [H2]Y where k = rate…

Q: Some measurements of the initial rate of a certain reaction are given in the table below. [N] N2 H,…

A: The question is placed on the concept of chemical kinetics. it makes use of initial rate law method…

Q: Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2…

Q: Consider the table of data collected for the reaction A → Products. Determine the magnitude (value)…

Question

Some measurements of the initial rate of a certain reaction are given in the table below.
N2|| |H2initial rate of reaction
1.21M 2.36M
5.00 x 10*M/s
1.21M| 0.916M
7.53 x 10° M/s
2.08M 2.36М
8.60 x 10“M/s
Use this information to write a rate law for this reaction, and calculate the value of the rate constant k.
Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol.
rate = k |||
x10
k =

Expert Solution

Step 1

Step by step

Solved in 3 steps with 3 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 the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s) Experiment 1 [A] (mol/L) Experiment 2 [A] (mol/L) 0 1.0 102 1.0 102 10. 8.4 103 5.0 103 20. 7.1 103 2.5 103 30. ? 1.3 103 40. 5.0 103 6.3 104 In Experiment 1, [B]0 = 10.0 M. In Experiment 2, [B]0 = 20.0 M. Rate=[A]t a. Use the concentration versus time data to determine the rate law for the reaction. b. Solve for the value of the rate constant (k) for the reaction. Include units. c. Calculate the concentration of A in Experiment 1 at t =30.s
Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?
A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
11.102 Suppose that you are studying a reaction and need to determine its rate law. Explain what you would need to measure in order to accomplish this in a single experiment, and how you could use graphical methods to get from the experimental data to a complete rate law.
. Account for the increase in reaction rate brought about by a catalyst.
For the reaction of crystal violet with NaOH(aq), the measured rate of reaction is 1.27 106 mol L1 s1 when the concentration of crystal violet cation is 4.13 105 mol/L. (a) Estimate how long it will take for the concentration of crystal violet to drop from 4.30 105 mol/L to 3.96 105 mol/L. (b) Could you use the same method to make an accurate estimate of how long it would take for the concentration of crystal violet to drop from 4.30 105 mol/L to 0.43 105 mol/L? Explain why or why not.
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
(Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a 10-K rise in temperature increases the reaction rate by two to four times. Use an average increase of three times to answer the questions below. (a) What is the approximate activation energy of a typical chemical reaction at 298 K? (b) If a catalyst increases a chemical reactions rate by providing a mechanism that has a lower activation energy, then what change do you expect a 10-K increase in temperature to make in the rate of a reaction whose uncatalyzed activation energy of 75 kJ/mol has been lowered to one half this value (at 298 K) by addition of a catalyst?
The type of rate law for a reaction, either the differential rate law or the integrated rate law, is usually determined by which data is easiest to collect. Explain.