Explanation (a) We have the following redox reaction : I − ( a q ) + N O 2 − → I 2 ( s ) + N O ( g ) Step 1: Separate the overall reaction into two half-reactions: one for oxidation and one for reduction. O x i d a t i o n : I − ( a q ) → I 2 ( s ) Reduction : N O 2 − ( s ) → N O ( g ) Step 2: Balance the elements, excluding H, O. O x i d a t i o n : 2 I − ( a q ) → I 2 ( s ) Reduction : N O 2 − ( s ) → N O ( g ) Step 3: Balance the elements H, O. O x i d a t i o n : 2 I − ( a q ) → I 2 ( s ) Reduction : N O 2 − ( s ) + 2 H + ( a q ) → N O ( g ) + H 2 O ( l ) In these half-reactions, all elements are balanced, including H, O. Hence, in the next step we need to balance the charge. Step 4: Balance each half-reaction with respect to charge by adding electrons. O x i d a t i o n : 2 I − ( a q ) → I 2 ( s ) + 2 e − Reduction : N O 2 − ( s ) + 2 H + ( a q ) + 1 e − → N O ( g ) + H 2 O ( l ) Step 5: Make the number of electrons in both half-reactions equal by multiplying one or both half reactions by a small whole number. O x i d a t i o n : [ 2 I − ( a q ) → I 2 ( s ) + 2 e − ] × 1 Reduction : [ N O 2 − ( s ) + 2 H + ( a q ) + 1 e − → N O ( g ) + H 2 O ( l ) ] × 2 Add these two reactions to get the balanced reaction. 2 N O 2 − ( s ) + 4 H + ( a q ) + 2 I − ( a q ) → 2 N O ( g ) + 2 H 2 O ( l ) + I 2 ( s ) (b) We have the following redox reaction: C l O 4 − ( a q ) + C l − ( a q ) → C l O 3 − ( a q ) + C l 2 ( g ) Step 1: Separate the overall reaction into two half-reactions: one for oxidation and one for reduction. O x i d a t i o n : C l − ( a q ) → C l 2 ( s ) Reduction : C l O 4 − ( a q ) → C l O 3 − ( a q ) Step 2: Balance the elements, excluding H, O. O x i d a t i o n : 2 C l − ( a q ) → C l 2 ( s ) Reduction : C l O 4 − ( a q ) → C l O 3 − ( a q ) Step 3: Balance the elements H, O. O x i d a t i o n : 2 C l − ( a q ) → C l 2 ( s ) Reduction : C l O 4 − ( a q ) + 2 H + ( a q ) → C l O 3 − ( a q ) + H 2 O ( l ) In these half-reactions, all elements are balanced, including H, O

Chemistry: A Molecular Approach & Student Solutions Manual for Chemistry: A Molecular Approach, Books a la Carte Edition Package

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ISBN: 9780321955517

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 18 Solutions

Chemistry: A Molecular Approach & Student Solutions Manual for Chemistry: A Molecular Approach, Books a la Carte Edition Package

Ch. 18 - Prob. 1SAQ Ch. 18 - Q2. Which statement is true for voltaic cells? a)...Ch. 18 - Prob. 3SAQ Ch. 18 - Prob. 4SAQ Ch. 18 - Prob. 5SAQ Ch. 18 - Prob. 6SAQ Ch. 18 - Q7. Use Table 18.1 to calculate G for the...Ch. 18 - Prob. 8SAQ Ch. 18 - Prob. 9SAQ Ch. 18 - Prob. 10SAQ

Ch. 18 - Prob. 11SAQ Ch. 18 - Prob. 12SAQ Ch. 18 - Prob. 13SAQ Ch. 18 - Prob. 14SAQ Ch. 18 - Q15. Which metal can be used as a sacrificial...Ch. 18 - 1. In electrochemistry, spontaneous redox...Ch. 18 - Prob. 2E Ch. 18 - Prob. 3E Ch. 18 - Prob. 4E Ch. 18 - Prob. 5E Ch. 18 - Prob. 6E Ch. 18 - Prob. 7E Ch. 18 - Prob. 8E Ch. 18 - Prob. 9E Ch. 18 - Prob. 10E Ch. 18 - Prob. 11E Ch. 18 - Prob. 12E Ch. 18 - Prob. 13E Ch. 18 - Prob. 14E Ch. 18 - 15. Is a spontaneous redox reaction obtained by...Ch. 18 - 16. How can Table 19.1 be used to predict whether...Ch. 18 - 17. Explain why , , and K are all interrelated. Ch. 18 - Prob. 18E Ch. 18 - Prob. 19E Ch. 18 - Prob. 20E Ch. 18 - Prob. 21E Ch. 18 - Prob. 22E Ch. 18 - 23. What are the anode and cathode reactions in a...Ch. 18 - Prob. 24E Ch. 18 - 25. What is a fuel cell? What is the most common...Ch. 18 - Prob. 26E Ch. 18 - 27. List some applications of electrolysis. Ch. 18 - Prob. 28E Ch. 18 - 29. What species is oxidized, and what species is...Ch. 18 - Prob. 30E Ch. 18 - Prob. 31E Ch. 18 - Prob. 32E Ch. 18 - Prob. 33E Ch. 18 - Prob. 34E Ch. 18 - Prob. 35E Ch. 18 - Prob. 36E Ch. 18 - Balance each redox reaction occurring in acidic...Ch. 18 - 38. Balance each redox reaction occurring in...Ch. 18 - Prob. 39E Ch. 18 - Prob. 40E Ch. 18 - 41. Balance each redox reaction occurring in basic...Ch. 18 - Prob. 42E Ch. 18 - 43. Sketch a voltaic cell for each redox reaction....Ch. 18 - 44. Sketch a voltaic cell for each redox reaction....Ch. 18 - Prob. 45E Ch. 18 - Prob. 46E Ch. 18 - 47. Consider the voltaic cell: a. Determine the...Ch. 18 - 48. Consider the voltaic cell: a. Determine the...Ch. 18 - 49. Use line notation to represent each...Ch. 18 - 50. Use line notation to represent each...Ch. 18 - Make a sketch of the voltaic cell represented by...Ch. 18 - 52. Make a sketch of the voltaic cell represented...Ch. 18 - 53. Determine whether or not each redox reaction...Ch. 18 - 54. Determine whether or not each redox reaction...Ch. 18 - 55. Which metal could you use to reduce Mn2+ ions...Ch. 18 - Prob. 56E Ch. 18 - Prob. 57E Ch. 18 - Prob. 58E Ch. 18 - Prob. 59E Ch. 18 - Prob. 60E Ch. 18 - Prob. 61E Ch. 18 - 62. Calculate for each balanced redox reaction...Ch. 18 - Prob. 63E Ch. 18 - 64. Which metal is the best reducing agent? a....Ch. 18 - 65. Use tabulated electrode potentials to...Ch. 18 - Prob. 66E Ch. 18 - 67. Calculate the equilibrium constant for each of...Ch. 18 - 68. Calculate the equilibrium constant for each of...Ch. 18 - Prob. 69E Ch. 18 - Prob. 70E Ch. 18 - Prob. 71E Ch. 18 - 72. Calculate and for a redox reaction with n =...Ch. 18 - 73. A voltaic cell employs the following redox...Ch. 18 - 74. A voltaic cell employs the redox reaction: 2...Ch. 18 - 75. An electrochemical cell is based on these two...Ch. 18 - Prob. 76E Ch. 18 - 77. A voltaic cell consists of a Zn/Zn2+ half-cell...Ch. 18 - 78. A voltaic cell consists of a Pb/Pb2+ half-cell...Ch. 18 - Prob. 79E Ch. 18 - Prob. 80E Ch. 18 - 81. A concentration cell consists of two Sn/Sn2+...Ch. 18 - Prob. 82E Ch. 18 - 83. Determine the optimum mass ratio of Zn to MnO2...Ch. 18 - 84. What mass of lead sulfate is formed in a...Ch. 18 - 85. Refer to the tabulated values of in Appendix...Ch. 18 - 86. Refer to the tabulated values of in Appendix...Ch. 18 - Prob. 87E Ch. 18 - Prob. 88E Ch. 18 - Prob. 89E Ch. 18 - Prob. 90E Ch. 18 - 91. Write equations for the half-reactions that...Ch. 18 - Prob. 92E Ch. 18 - 93. Write equations for the half-reactions that...Ch. 18 - 94. What products are obtained in the electrolysis...Ch. 18 - 95. Write equations for the half-reactions that...Ch. 18 - Prob. 96E Ch. 18 - 97. Make a sketch of an electrolysis cell that...Ch. 18 - Prob. 98E Ch. 18 - Prob. 99E Ch. 18 - Prob. 100E Ch. 18 - Prob. 101E Ch. 18 - Prob. 102E Ch. 18 - 105103. Consider the unbalanced redox...Ch. 18 - Prob. 104E Ch. 18 - 107. Consider the molecular views of an Al strip...Ch. 18 - 106. Consider the molecular view of an...Ch. 18 - Prob. 107E Ch. 18 - Prob. 108E Ch. 18 - Prob. 109E Ch. 18 - Prob. 110E Ch. 18 - Prob. 111E Ch. 18 - Prob. 112E Ch. 18 - Prob. 113E Ch. 18 - Prob. 114E Ch. 18 - Prob. 115E Ch. 18 - Prob. 116E Ch. 18 - 119. The Ksp of CuI is 1.1 × 10–12. Find Ecell for...Ch. 18 - 120. The Ksp of Zn(OH)2 is 1.8 × 10–14. Find Ecell...Ch. 18 - 121. Calculate and K for each reaction. a. The...Ch. 18 - Prob. 120E Ch. 18 - Prob. 121E Ch. 18 - Prob. 122E Ch. 18 - Prob. 123E Ch. 18 - Prob. 124E Ch. 18 - Prob. 125E Ch. 18 - Prob. 126E Ch. 18 - Prob. 127E Ch. 18 - 130. To what pH should you adjust a standard...Ch. 18 - 131. Suppose a hydrogen–oxygen fuel-cell generator...Ch. 18 - 132. A voltaic cell designed to measure [Cu2+] is...Ch. 18 - 133. The surface area of an object to be gold...Ch. 18 - Prob. 132E Ch. 18 - Prob. 133E Ch. 18 - Prob. 134E Ch. 18 - Prob. 135E Ch. 18 - Prob. 136E Ch. 18 - Prob. 137E Ch. 18 - 140. A redox reaction employed in an...Ch. 18 - 141. A redox reaction has an equilibrium constant...

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