Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
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Chapter 13, Problem 13.21QE
(a)
Interpretation Introduction
Interpretation:
An expression for the
(b)
Interpretation Introduction
Interpretation:
The average rate of reaction between 10 and 30 seconds has to be calculated.
(c)
Interpretation Introduction
Interpretation:
The instantaneous of reaction after 20 sec has to be determined.
(d)
Interpretation Introduction
Interpretation:
The initial rate of reaction has to be determined.
(e)
Interpretation Introduction
Interpretation:
The instantaneous rate of formation of
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Consider this balanced chemical equation:H2O2(aq) + 3 I - (aq) + 2 H+ (aq)------> I3 - (aq) + 2 H2O(l )In the first 10.0 seconds of the reaction, the concentration of I - drops from 1.000 M to 0.868 M.(a) Calculate the average rate of this reaction in this time interval.(b) Determine the rate of change in the concentration of H+ (that is, Δ[H+]>Δt) during this time interval.
1. Which of the following statements is incorrect?
(A) As the chemical reaction proceeds, the rate of reaction increases.
(B) The reaction rate almost gets doubled for 10°C rise in temperature.
(C) For a first order chemical reaction, the rate constant has unit of time-1.
(D) Chemical kinetics can predict the rate of a chemical reaction.
2. In a chemical reaction, represented by A → P, it is observed that the rate of reaction increases by a
factor of 4 on doubling the concentration of the reactant. The rate of reaction increases by a factor of 9 on
trebling the concentration of the reactant. Then the rate of the reaction is proportional to
(A) CA
(B) CA2
(C) CA3
(D) CA4
3. An elementary reaction has the stoichiometric equation A + 2B = P. What is the order of reaction
(A) 0
(B) 1
(C) 2
(D) 3
4. It states that the rate of a chemical reaction is directly proportional to the product of the activities or
concentrations of the reactants.
(A) Law of mass action…
Consider the following reaction:
1.
2 N,O5 (g) → 4 NO, (g) + O, (g)
The initial concentration of N2O5 was 0.48
mol/L, and 25 minutes after initiating the
reaction, all of the N,Os has been consumed.
(a) Calculate the average rate of the reaction
over this 25-minute time interval.
(b) Is it correct to assume that the rate law is
Rate = k[N,O5]² based on the balanced
chemical equation? Briefly explain your
answer.
Chapter 13 Solutions
Chemistry: Principles and Practice
Ch. 13 - Prob. 13.1QECh. 13 - Prob. 13.2QECh. 13 - What is the difference between the integrated and...Ch. 13 - Prob. 13.4QECh. 13 - Explain why half-lives are not normally used to...Ch. 13 - Derive an expression for the half-life of a...Ch. 13 - Prob. 13.7QECh. 13 - Prob. 13.8QECh. 13 - Prob. 13.9QECh. 13 - Prob. 13.10QE
Ch. 13 - Prob. 13.11QECh. 13 - Prob. 13.12QECh. 13 - Prob. 13.13QECh. 13 - Prob. 13.14QECh. 13 - Prob. 13.15QECh. 13 - Prob. 13.16QECh. 13 - Prob. 13.17QECh. 13 - Prob. 13.18QECh. 13 - Prob. 13.19QECh. 13 - Prob. 13.20QECh. 13 - Prob. 13.21QECh. 13 - Prob. 13.22QECh. 13 - Nitrogen monoxide reacts with chlorine to form...Ch. 13 - Prob. 13.24QECh. 13 - Prob. 13.25QECh. 13 - Prob. 13.26QECh. 13 - Prob. 13.27QECh. 13 - Prob. 13.28QECh. 13 - Prob. 13.29QECh. 13 - Prob. 13.30QECh. 13 - Prob. 13.31QECh. 13 - Prob. 13.32QECh. 13 - Prob. 13.33QECh. 13 - Write a rate law for NO3(g) + O2(g) NO2(g) +...Ch. 13 - Prob. 13.35QECh. 13 - Prob. 13.36QECh. 13 - Prob. 13.37QECh. 13 - Rate data were obtained at 25 C for the following...Ch. 13 - Prob. 13.39QECh. 13 - Prob. 13.40QECh. 13 - Prob. 13.41QECh. 13 - Prob. 13.42QECh. 13 - Prob. 13.43QECh. 13 - Prob. 13.44QECh. 13 - Prob. 13.45QECh. 13 - Prob. 13.46QECh. 13 - Prob. 13.47QECh. 13 - Prob. 13.48QECh. 13 - When formic acid is heated, it decomposes to...Ch. 13 - Prob. 13.50QECh. 13 - The half-life of tritium, 3H, is 12.26 years....Ch. 13 - Prob. 13.52QECh. 13 - Prob. 13.53QECh. 13 - Prob. 13.54QECh. 13 - Prob. 13.55QECh. 13 - Prob. 13.56QECh. 13 - The decomposition of ozone is a second-order...Ch. 13 - Prob. 13.58QECh. 13 - Prob. 13.59QECh. 13 - Prob. 13.60QECh. 13 - A reaction rate doubles when the temperature...Ch. 13 - Prob. 13.62QECh. 13 - Prob. 13.63QECh. 13 - Prob. 13.64QECh. 13 - Prob. 13.65QECh. 13 - The activation energy for the decomposition of...Ch. 13 - Prob. 13.67QECh. 13 - Prob. 13.68QECh. 13 - Prob. 13.69QECh. 13 - Prob. 13.70QECh. 13 - Prob. 13.71QECh. 13 - Prob. 13.72QECh. 13 - Prob. 13.73QECh. 13 - Prob. 13.74QECh. 13 - Prob. 13.75QECh. 13 - Prob. 13.76QECh. 13 - Prob. 13.77QECh. 13 - Prob. 13.78QECh. 13 - Prob. 13.79QECh. 13 - Prob. 13.80QECh. 13 - The gas-phase reaction of nitrogen monoxide with...Ch. 13 - Prob. 13.82QECh. 13 - Prob. 13.83QECh. 13 - A catalyst reduces the activation energy of a...Ch. 13 - Prob. 13.85QECh. 13 - Prob. 13.86QECh. 13 - Prob. 13.87QECh. 13 - Prob. 13.88QECh. 13 - Prob. 13.89QECh. 13 - Prob. 13.90QECh. 13 - Prob. 13.91QECh. 13 - Prob. 13.92QECh. 13 - Prob. 13.93QECh. 13 - Prob. 13.94QECh. 13 - Prob. 13.95QECh. 13 - Prob. 13.96QECh. 13 - Prob. 13.98QECh. 13 - Prob. 13.99QE
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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
- The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?arrow_forwardConsider 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.arrow_forward. Account for the increase in reaction rate brought about by a catalyst.arrow_forward
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