5. The reaction A products is a second-order reaction and takes place at 32°C. a. Given that the half-life of this reaction is 4.22 x 104 s when the initial concentration of A is 0.2 M, what is the rate constant for the reaction? Include units with your answer. b. At 305 K, how long will it take for a 0.028 M sample of A to decrease to 0.0042 M? c. Initially 4.00 mol of A is placed in a 6.00 L container and allowed to react. How many moles of A would remain after 24.0 hours? Assume the temperature is 32 °C.

5. The reaction A products is a second-order reaction and takes place at 32°C. a. Given that the half-life of this reaction is 4.22 x 104 s when the initial concentration of A is 0.2 M, what is the rate constant for the reaction? Include units with your answer. b. At 305 K, how long will it take for a 0.028 M sample of A to decrease to 0.0042 M? c. Initially 4.00 mol of A is placed in a 6.00 L container and allowed to react. How many moles of A would remain after 24.0 hours? Assume the temperature is 32 °C.

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

The half-life for the first-order conversion of A to B is 56.5 hours. How long does it take for the concentration of A to decrease to 10.0% of its original concentration? O a. 565 hr O b.0.111 hr Oc. 56.5 hr O d.0.123 hr O e. 188 hr е.
The decomposition of gaseous dinitrogen pentaoxide (N2O5) to NO2 and O2 is a first-order reaction. At 60°C the half-life of the reaction is 2.48 x 102 s. If the initial concentration of N2O5 is 1.58 mol/L, then: a. What is [N2O5] after 3 minutes? b. What fraction of N2O5 has decomposed after 3 minutes?
IX. Derive the half-life equation for a zero-order reaction. What is the half-life for the decomposition of a sample with a measured rate constant of 1.44 mol L-1 s-1 and an initial concentration of 92.2 mol/L. Round your answer to 2 decimal places.
The half-life of a first order reaction is constant and equal to 0.693/k. CA first order reaction with k= 3.465 x 10-2 s-1 is started with [A]o=0.800 M. What is the concentration of A after 60 seconds? Oa. 0.100 M Ob. 0.400 M Oc. c. 0.200 M Od. 0.0800 M
Half-life of a reaction The order of the reaction, ? → products, is being determined through the half-life method. Two setups at the same temperatures but different starting concentrations of A were investigated. For the first run, the initial concentration of A was 0.78 M and the halflife was determined to be 45 minutes. In the second run, the initial concentration of A was 1.32 M. Determine the following : a. If the reaction is 1st order, what should be the half-life of the second run in minutes? b. If the reaction is 2nd order, what should be the half-life of the second run in minutes? c. If the reaction is 0th order, determine the concentration of A in the second run after 152.3 minutes.
Derive the half-life equation for a zero-order reaction. What is the half-life for the decomposition of a sample with a measured rate constant of 9.8 mol L-1 s-1 and an initial concentration of 80.66 mol/L. Round your answer to 2 decimal places.
Consider the reaction A > B. The initial [A] is 0.10 M. After 1.0 hour, 50% of A has reacted. a. Draw a graph of concentration vs. time for each of the cases below. i. The reaction is zero order in A. I. The reaction is first order in A. b. Predict what the concentration of A will be after 2.0 hours for each case in part a if the initial [A] were 0.050 M. Explain your reasoning.
Molecular iodine, I2 (g), dissociates into iodine atoms at 652 K, with a first order rate constant of 0.452 s-1. I2(g) -----> 2I a. What is the half life for this reaction? b. If you start with 0.35 M I2 at this temperature, how long will it take for the concentration of I2 to reach 0.12 M?
Derive the half-life equation for a second-order reaction. What is the half-life for the decomposition of a sample with a measured rate constant of 1.57 L mol-1 s-1 and an initial concentration of 91.27 mol/L. Round your answer to 2 decimal places.
16. What data should be plotted to show that experimental concentration data fits a second-order reaction? A. ln[reactant] vs. time B. [reactant] vs. time C. ln(k) vs. 1/T D. 1/[reactant] vs. time F. ln(k) vs. Ea
For the reaction below, a series of experiments was conducted and the data collected in the table below. a. Determine the rate law and the overall order of the reaction. b. Calculate the rate constant, including appropriate units. c. Determine the initial rate when the initial concentrations of both reactants are 0.12 M. Reaction (might be unbalanced): NO (g) + Cl2 (g) → NOCI (g) Experiment Data: Experiment # Initial [NO] (M) Initial [Cl2] (M) Initial Rate (M/s) 0.13 1.0x10-2 0.20 2 0.26 0.20 4.0x10-2 3 5.0x10-3 0.13 0.10
10. For first order reaction A →P with rate constant k = 0.02 s' , how long it would for concentration of A to fall from 0.5M to 0.0005 M? What is half-life of this reaction?