Your laboratory is asked to analyze a water sample for a particular pesticide. You knowfrom previous study that this pesticide degrades via a first order, irreversible reaction. Thefirst order rate constant (k) for the reaction at 4 °C is 0.02 day¹. The activation energy forthe reaction is known to be 10 kcal/mol. The standard preservation method for watersamples containing this pesticide is to store the sample at 4 °C for no more than 24 hoursprior to analysis.Calculate the fraction of the pesticide that remains in the sample after 24 hours of storageat 4 °C.b. A newly hired staff member collects a sample of the water but forgets to store it at 4 °C.Instead, they leave the sample in the trunk of their car (average temperature 35 °C) overthe weekend. 60 hours later the sample is analyzed and found to contain 0.01 mg/L ofthe pesticide. What was the pesticide concentration in the water at the time the samplewas taken?

a) Here initial concentration (t=0) of pesticide is a0. After time 24 hrs (t1) the concentration of…

Your laboratory is asked to analyze a water sample for a particular pesticide. You know from previous study that this pesticide degrades via a first order, irreversible reaction. The first order rate constant (k) for the reaction at 4 °C is 0.02 day. The activation energy for the reaction is known to be 10 kcal/mol. The standard preservation method for water samples containing this pesticide is to store the sample at 4 °C for no more than 24 hours prior to analysis. a. Calculate the fraction of the pesticide that remains in the sample after 24 hours of storage at 4 °C. b. A newly hired staff member collects a sample of the water but forgets to store it at 4 °C. Instead, they leave the sample in the trunk of their car (average temperature 35 °C) over the weekend. 60 hours later the sample is analyzed and found to contain 0.01 mg/L of the pesticide. What was the pesticide concentration in the water at the time the sample was taken?

Your laboratory is asked to analyze a water sample for a particular pesticide. You know from previous study that this pesticide degrades via a first order, irreversible reaction. The first order rate constant (k) for the reaction at 4 °C is 0.02 day. The activation energy for the reaction is known to be 10 kcal/mol. The standard preservation method for water samples containing this pesticide is to store the sample at 4 °C for no more than 24 hours prior to analysis. a. Calculate the fraction of the pesticide that remains in the sample after 24 hours of storage at 4 °C. b. A newly hired staff member collects a sample of the water but forgets to store it at 4 °C. Instead, they leave the sample in the trunk of their car (average temperature 35 °C) over the weekend. 60 hours later the sample is analyzed and found to contain 0.01 mg/L of the pesticide. What was the pesticide concentration in the water at the time the sample was taken?

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

A chemistry graduate student is studying the rate of this reaction: NH,ОH (аq) — NH; (аq)+ н,о (аq) She fills a reaction vessel with NH,OH and measures its concentration as the reaction proceeds: time [NH,OH] (seconds) 0.0600M 0.10 0.0385 M 0.20 0.0247M 0.30 0.0158M 0.40 0.0101 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k || x10 Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
1) For a particular chemical reaction, the rate constant at 30.0 °C is 1.38 x 10-4 L mol-1 s-1, while the value at 49.0 °C is 1.21 x 10-3 L mol-1 s-1. What is the activation energy for this reaction? A) 200 kJ mol-1 B) 343 kJ mol-1 C) 40.4 kJ mol-1 D) 56.4 kJ mol-1 1)
Which of the following statements is true? A catalyst raises the activation energy of a reaction. The addition of a homogeneous catalyst does not change the activation energy of a given reaction. The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants. Rate constants are temperature dependent. None of the above are true.
A chemistry graduate student is studying the rate of this reaction: 2HI (g) → H₂ (g) +1₂ (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [HI] 0.0400M 0.0199M 0.20 0.0133 M 0.30 0.00994M 0.40 0.00795 M Use this data to answer the following questions. Write the rate law for this reaction. 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. rate = k k = 0 x10 X Ś
The rate of a certain reaction was studied at various temperatures. The table shows temperature (?) and rate constant (?) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, ?a , for this reaction? What is the value of the pre‑exponential factor (sometimes called the frequency factor), ? , for this reaction? Temperature (K) k (s^-1) 400 0.0000173 580 7.43
Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation. 2 HI(g) → H2(g) + I2(g) At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 M to 3.50 × 10-2 M. What is the rate constant for the reaction at this temperature?
A student collected conducted 6 kinetics experiments for one reaction by holding the concentrations of ALL the reactants and catalyst constant and varying the temperature. After determining the rate constant for this reaction at the 6 different temperatures, an Arrhenius Plot was made. The graph resulted in a straight line. The equation for the straight line was: y= -3,378.84 x + 14.326 What is the Activation Energy (in Joules/mol) for this reaction at 30 oC? Do not include the units in your answer.
An energy diagram showing two peaks suggests that there are two steps and three transition states in the reaction mechanism. Select one: O True O False Given a reaction with an activation energy of 2.3 x 104 J/mol. The rate constant will increase by a factor of when the reaction temperature is increased from 200 °C to 250 °C. O 2.42 O 2.81 O 1.58 O 1.75 For the complete neutralization reaction between a 1 M strong acid and a 1 M strong base of equal initial volumes that is marked by a temperature rise, the entropy of neutralization is positive (ASn > 0) whereas the Gibbs free energy is negative (AGxn < 0). Select one: O True O False
A certain 2nd order reaction is known to proceed by a two-step process such that k1<<k2. The forward reaction has an activation energy of 48 kJ/mole and the reverse reaction has an activation energy of 62 kJ/mole. Sketch the energy diagram for the reaction.
The rate constant for a reaction varies between 0.590 L·mol-1·s-1 at 325°C and 2.10 L·mol-1·s-1 at 400°C. Determine the activation energy for this reaction to the nearest whole number in units of kilojoules per mole. Include only the numerical answer (no units).
A chemistry graduate student is studying the rate of this reaction: 2C1₂O5 (g) → 2Cl₂ (g) +50₂ (g) He fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [C₁₂05] 0.600M 0.215M 0.20 00. 0.131M 0.30 0.0941 M 0.40 0.0734M Use this data to answer the following questions. Write the rate law for this reaction. 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. rate k = - k 0 ☐x10 X Ś
For a particular reaction, the rate constant k is 2.8 × 10-5 L mol-1 s-1 at 27 ℃ and 7.0 × 10-5 L mol-1 s-1 at 227 ℃. Calculate the activation energy for the reaction.