Consider the reaction: A → B.Use the below data to determine the second half-life for experiment 2. Please answer in seconds.Experiment25012[A]0.1 M0.2 MInitial Rate [M/S]0.00250.01Incorrect. We learned in the previous problems that this reaction is second order and k = 0.25 M²¹ s²¹.During the first half-life, [A] decreases by 50% (0.2 M to 0.1M). Now we need to determine how long it will take for [A] decrease byanother 50% (0.1 M to 0.05 M). This means the original concentration for the second half-life of experiment #2 is 0.1 M. Consider the reaction: A → B.Use the below data to determine the first half-life for experiment 1. Please answer in seconds.[A]Experiment4,00012Incorrect.0.1 M0.2 MInitial Rate [M/S]0.00250.01When we double the concentration of A, the rate quadruples. This means that this reaction is second order. Make sure you are usingthe correct half-life equation!*Check to make sure you are using the data from Experiment #1.

Answered: Image /qna-images/answer/ae2e0fc8-151a-4f62-85c3-f98d4e73f18a.jpg

Consider the reaction: A → B. Use the below data to determine the first half-life for experiment 1. Please answer in seconds. Initial Rate [M/s] Experiment 4,000 1 2 Incorrect. [A] 0.1 M 0.2 M 0.0025 0.01

Consider the reaction: A → B. Use the below data to determine the first half-life for experiment 1. Please answer in seconds. Initial Rate [M/s] Experiment 4,000 1 2 Incorrect. [A] 0.1 M 0.2 M 0.0025 0.01

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

Similar questions

Please complete answers 30 mint asap
Question 11 of 19 What is the half-life for a particular reaction if the rate law is rate= (901 min-¹) [A]? Tap here or pull up for additional resources MacBook Air 1 4 7 +/- 2 min 8 3 5 6 SOSO 9 Submit x C x 100
Please explain after answering
Determine the average rate of change of B from t = 0 s to = 362 s. A → 2B rate = M/s Time (s) 0 181 362 Concentration of A (M) 0.720 0.425 0.130
A general reaction written as A + 2B → C + 2D is studied and yields the following data: rate of formation of C is A[C]/At = 8.00 x 10-3 M/s Determine the rate of consumption of B, -A[B]/At = %3D a. 4.00 x 10-3 M/s b. 8.00 x 10-3 M/s c. 32.00 x 10-3 M/s d. 16.00 x 10-3 M/s
. For the following generic reaction: a A + b B -- > c C + d DWhat is the rate of reaction (rate expression) as a function of change in concentration (e.g. Δ[A]) andchange in time (Δt)?Describing Chemical Kinetics:1. Measuring RateThe rate of a chemical reaction is determined by:A. Change of moles of reactants/products over change in timeB. Change of grams of reactants/products over change in timeC. Change in concentration over change in timeD. change in volume over change in timeWrite the rate expressions based on the definition above for:a A + b B -- > c C + d Da A -- > productsDoes the order in reactant (m, n) in the rate law have anything to do with the coefficients of the reactants?
43-46 Consider the time and concentration data for: 2 NO2(g) 2 NO(g) + O2(g). Time, s [NO2] 43 a. How long is the first half-life? Write the value and units 0.100 0.072 20 b. How long is the second half-life? Write the value and units 0.050 50 44. Write the rate law for this reaction. Explain why you made this choice. 0.036 90 0.025 150 45. What is the value of the rate constant? Write the general equation, the calculation equation with units, and the answer with units 46. How much time is needed until only 0.010 M NO2 remains? Write the general equation, the calculation with units, and the answer with units c
[A] vs Time In[A] vs Time O 1/[A] vs Time Least Squares Plot The reaction A → C was performed and the concentration vs. time data below collected. time, s [A], mol/L 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 0.03405 0.02995 [A] 0 reaction order = Check Submit Answer 1 Time, s 2 3 Try Another Version Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = Next> (1 of 1) Show Approach 2 item att 5 6 Hide Hint 7 8 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.
A particular reactant decomposes with a half-life of 121 s when its initial concentration is 0.354 M. The same reactant decomposes with a half-life of 239 s when its initial concentration is 0.179 M. Determine the reaction order. 01 What is the value and units of the rate constant for this reaction? Units 0.17 Enter numeric value TOOLS x10
The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H Iz + 2 HCI Initial Rate, Ms! 1.57x10-2 3.13×10-2 6.24x10-2 0.125 Experiment [ICI]. M H), M 1 0.207 0.211 2 0.414 0.211 3 0.207 0.421 4 0.414 0.421 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is
Use the graph to answer the questions below. Report answers to 3 significant figures. a. What is the initial concentration? b. What is the concentration at 1250 seconds? c. At what time is the concentration .0167M? d. What is the half-life? e. What is the rate constant? 7. a. Calculate the enthalpy of the reaction H2C=CH2(g) + H2O(ℓ) →CH3−CH2−OH(ℓ)