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Ch.14 - Chemical Kinetics
Chapter 14, Problem 40

The decomposition of sodium bicarbonate (baking soda), NaHCO31s2, into Na2CO31s2, H2O1l2, and CO21g2 at constant pressure requires the addition of 85 kJ of heat per two moles of NaHCO3. (b) Draw an enthalpy diagram for the reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Decomposition Reaction

A decomposition reaction is a type of chemical reaction where a single compound breaks down into two or more simpler products. In this case, sodium bicarbonate (NaHCO3) decomposes into sodium carbonate (Na2CO3), water (H2O), and carbon dioxide (CO2). Understanding this concept is crucial for analyzing the reaction's products and the energy changes involved.
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Enthalpy Change (ΔH)

Enthalpy change, represented as ΔH, is the heat content change of a system at constant pressure. In this reaction, the addition of 85 kJ of heat indicates that the process is endothermic, meaning it absorbs heat from the surroundings. This concept is essential for understanding how energy is transferred during the reaction and for drawing the enthalpy diagram.
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Enthalpy Diagram

An enthalpy diagram visually represents the energy changes during a chemical reaction. It typically shows the enthalpy of reactants and products, along with the energy required for the reaction to proceed. For the decomposition of sodium bicarbonate, the diagram will illustrate the initial and final energy states, highlighting the endothermic nature of the reaction and the heat absorbed.
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Related Practice
Textbook Question

Consider the gas-phase reaction between nitric oxide and bromine at 273 C: 2 NO1g2 + Br21g2¡2 NOBr1g2. The following data for the initial rate of appearance of NOBr were obtained: Experiment 3no4 1M 2 3br2 4 1M 2 Initial Rate 1M,s2 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 (b) Calculate the average value of the rate constant for the appearance of NOBr from the four data sets.

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Textbook Question

Consider the reaction of peroxydisulfate ion 1S2O82-2 with iodide ion 1I - 2 in aqueous solution: S2O8 2 - 1aq2 + 3 I - 1aq2¡2 SO42 - 1aq2 + I3- 1aq2 At a particular temperature, the initial rate of disappearance of S2O82 - varies with reactant concentrations in the following manner: Experiment 3S2o8 24 1M 2 3I4 1M 2 Initial Rate 1M,s2 1 0.018 0.036 2.6 * 10-6 2 0.027 0.036 3.9 * 10-6 3 0.036 0.054 7.8 * 10-6 4 0.050 0.072 1.4 * 10-5 (a) Determine the rate law for the reaction and state the units of the rate constant.

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Textbook Question

(a) For the generic reaction A S B what quantity, when graphed versus time, will yield a straight line for a first-order reaction?

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Textbook Question

(a) The gas-phase decomposition of SO2Cl2, SO2Cl21g2 ¡SO21g2 + Cl21g2, is first order in SO2Cl2. At 600 K the half-life for this process is 2.3 * 105 s. What is the rate constant at this temperature?

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Textbook Question

As described in Exercise 14.41, the decomposition of sulfuryl chloride 1SO2Cl22 is a first-order process. The rate constant for the decomposition at 660 K is 4.5 * 10-2 s-1. (b) At what time will the partial pressure of SO2Cl2 decline to one-tenth its initial value?

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Textbook Question

The first-order rate constant for the decomposition of N2O5, 2 N2O51g2¡4 NO21g2 + O21g2, a t 70 C i s 6.82 * 10-3 s-1. Suppose we start with 0.0250 mol of N2O51g2 in a volume of 2.0 L. (a) How many moles of N2O5 will remain after 5.0 min?

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