5.The reaction A →→ B + C is known to be first order in A. Below are data showing the concentration of Aas a function of reaction time.Time, h012481012[A]. M1.50 x 10-¹1.27 x 10-11.07 x 10-17.66 x 10-²3.91 x 10-²2.80 x 10-22.00 x 10-2(a) What is the average rate of reaction between 1 and 4 h? Report the units as well as the numbers.(b) Plot the data above, showing the concentration of A as a function of the time. From your graph,determine the instantaneous rate of reaction at 8 h. Report the units as well as the numbers.(c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph.Report the units as well as the numbers.

The given first order reaction is :A → B + CThe data showing change in concentration of A with…

12 2.00 x 10-2 (a) What is the average rate of reaction between 1 and 4 h? Report the units as well as the (b) Plot the data above, showing the concentration of A as a function of the time. From you ne the instantaneous rate of reaction at 8 h. Report the units as well as the numbers. (c) Plot In [A] versus time Estimate the rate constant for this first-order reaction from your

12 2.00 x 10-2 (a) What is the average rate of reaction between 1 and 4 h? Report the units as well as the (b) Plot the data above, showing the concentration of A as a function of the time. From you ne the instantaneous rate of reaction at 8 h. Report the units as well as the numbers. (c) Plot In [A] versus time Estimate the rate constant for this first-order reaction from your

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

[3] Nitrogen dioxide gas (NO2) decomposes slowly to nitrous oxide (NO) and oxygen (O,) at 383 °C. At 383 °C the concentration verses time data were collected for this reaction, and a plot of 1/[NO2] verses time resulted in a straight line with a slope of 4.7/M-s. If the initial concentration of NO2 = 0.600M. (a) Determine the rate law. (b) Determine the value of the rate constant, k. (c) How long will it take for 40 % the NO, to be converted to product?
Using the half-life method, the order of the reaction A ---> products is being analyzed. There are two identical temperatures but different initial concentrations of A. For first trial, the starting concentration of A is 0.78 M and its half-life was analyzed to be 45 mins. For the second trial, the starting concentration of A is 1.32 M. Given these observation, What should be the half-life of the second trial (minutes), if the reaction is in first order? What should be the half-life of the second trial (minutes), if the reaction is in second order? Calculate the concentration of A in the second trial after 152.3 minutes, if the reaction is in zeroth order?
Which of the following judgments about the value of the rate order of the reaction is correct? I) If the rate order is zero; the doubling of the reactant concentration does not affect the initial reaction rate. II) If the first order; the doubling of the reactant concentration doubles the initial rate of the reaction. III) If the reaction is second-order; increasing the reactant concentration by 2 times increases the reaction rate by 4 times. IV) The plot of each reaction rate order should be linear, even the value of the slope is negative or positive.
None
. [Template] Kinetic... > Homework (2) : In second order reaction It is found that 20% in convert to product during 40 minutes. When the reaction starts at a concentration equal to 0.1 M, calculate the following: (A) The reaction rate constant (B) Half-life of the reaction (C) Time to complete 20% of the reaction when the initial concentration is 0.01 M II
sub= 9
Answer Q
phy chem 1
A first-order reaction has a rate constant of 3.6 x 10-3s-1. How many seconds does it take for the reaction to be 31.3% complete? (Report an integer)
ZAIN IQ all all EM N96% 4,18 ZAIN IQ + [Template] Kin.. / Homework (2) : In second order reaction It is found that 20% in convert to product during 40 minutes. When the reaction starts at a concentration equal to 0.1 M, calculate the following: (A) The reaction rate constant (B) Half-life of the reaction (C) Time to complete 20% of the reaction when the initial concentration is 0.01 M
The reaction of IC1 with hydrogen 2IC1 + H₂ → I2 + 2HCl is first order in IC1 and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' 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 =
The reaction 2A → B is second order with a rate constant of 51.0/M-min at 24°C. (a) Starting with [A]o = 9.50× 10-3 M, how long will it take for [A]ƒ = 2.80 × 10-3 M? min (b) Calculate the half-life of the reaction. = min