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 13.65QE
Interpretation Introduction
Interpretation:
The factor does the
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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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- Nitrosyl bromide, NOBr, is formed from NO and Br2: 2 NO(g) + Br2(g) 2 NOBr(g) Experiments show that this reaction is second-order in NO and first-order in Br2. (a) Write the rate equation for the reaction. (b) How does the initial reaction rate change if the concentration of Br2 is changed from 0.0022 mol/L to 0.0066 mol/L? (c) What is the change in the initial rate if the concentration of NO is changed from 0.0024 mol/L to 0.0012 mol/L?arrow_forwardAt 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.arrow_forwardOzone, O3, in the Earths upper atmosphere decomposes according to the equation 2 O3(g) 3 O2(g) The mechanism of the reaction is thought to proceed through an initial fast, reversible step followed by a slow, second step. Step 1: Fast, reversible O3(g) O2(g) + O(g) Step 2: Slow O3(g) + O(g) 2 O2(g) (a) Which of the steps is rate-determining? (b) Write the rate equation for the rate-determining steparrow_forward
- Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?arrow_forwardThe decomposition of iodoethane in the gas phase proceeds according to the following equation: C2H5I(g)C2H4(g)+HI(g) At 660. K, k = 7.2 104 sl; at 720. K, k = 1.7 102 sl. What is the value of the rate constant for this first-order decomposition at 325C? If the initial pressure of iodoethane is 894 torr at 245C, what is the pressure of iodoethane after three half-lives?arrow_forwardConsider the hypothetical reaction A2(g) + B2(g) 2AB(g), where the rate law is: [A2]t=k[A2][B2] The value of the rate constant at 302C is 2.45 104 L/mol s, and at 508C the rate constant is 0.891 L/mol s. What is the activation energy for this reaction? What is the value of the rate constant for this reaction at 375C?arrow_forward
- The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) 2 HI(g)Rate = k[H2][I2] Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. (a) The reaction must occur in a single step. (b) This is a second-order reaction overall. (c) Raising the temperature will cause the value of k to decrease. (d) Raising the temperature lowers the activation energy for this reaction. (e) If the concentrations of both reactants are doubled, the rate will double. (f) Adding a catalyst in the reaction will cause the initial rate to increase.arrow_forward11.44 A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 4.0 X 10_H s"' at 25°C. What is the half-life for the degradation of DDT in this experiment, in years?arrow_forwardThe following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.arrow_forward
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