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Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus ISBN: 9780134414232 1274

Solution for problem 4.55 Chapter 4

Chemistry: The Central Science | 14th Edition

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Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

Chemistry: The Central Science | 14th Edition

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Problem 4.55 Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Iron metal is added to a solution of copper(II) nitrate, (b) zinc metal is added to a solution of magnesium sulfate, (c) hydrobromic acid is added to tin metal,(d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride, (e) aluminum metal is added to a solution of cobalt(II) sulfate.
Step-by-Step Solution:

Step 1 of 5) Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR.If the total enthalpy of the broken bonds is larger, the reaction is endothermic 1∆Hrxn 7 02; if the total enthalpy of the newly formed bonds is larger, the reaction is exothermic 1∆Hrxn 6 02. Consider for example, the gas-phase reaction between methane, CH4, and chlorine to produce methyl chloride, CH3Cl, and hydrogen chloride, HCl: H¬CH31g2 + Cl¬Cl1g2 ¡ Cl¬CH31g2 + H¬Cl1g2 ∆Hrxn = [5.33] Our two-step procedure is outlined in Figure 5.24. We note that the following bonds are broken and formed:We first supply enough energy to break the C—H and Cl—Cl bonds, which raises the enthalpy of the system (indicated as ∆H1 7 0 in Figure 5.24). We then form the C—Cl and H—Cl bonds, which release energy and lower the enthalpy of the system (∆H2 6 0 in Figure 5.24). We then use Equation 5.32 to estimate the enthalpy of the reaction: ∆Hrxn = 3D1C¬H2 + D1Cl¬Cl24 - 3D1C¬Cl2 + D1H¬Cl24 ∆Hrxn = 1413 kJ + 242 kJ2 - 1328 kJ + 431 kJ2 = -104 kJ The reaction is exothermic because the bonds in the products are stronger than the bond in the reactants. Typically, bond enthalpies are used to estimate ∆Hrxn only if the needed ∆Hf° values are not readily available. For the preceding reaction, we cannot calculate ∆Hrxn from ∆Hf

Step 2 of 2

Chapter 4, Problem 4.55 is Solved
Textbook: Chemistry: The Central Science
Edition: 14
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
ISBN: 9780134414232

The answer to “Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Iron metal is added to a solution of copper(II) nitrate, (b) zinc metal is added to a solution of magnesium sulfate, (c) hydrobromic acid is added to tin metal,(d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride, (e) aluminum metal is added to a solution of cobalt(II) sulfate.” is broken down into a number of easy to follow steps, and 72 words. Since the solution to 4.55 from 4 chapter was answered, more than 212 students have viewed the full step-by-step answer. The full step-by-step solution to problem: 4.55 from chapter: 4 was answered by , our top Chemistry solution expert on 10/03/18, 06:29PM. Chemistry: The Central Science was written by and is associated to the ISBN: 9780134414232. This full solution covers the following key subjects: . This expansive textbook survival guide covers 29 chapters, and 1665 solutions. This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 14.

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