Interpretation Introduction Introduction: The entropy change of surroundings ( Δ S s u r r ) is negative of the ratio of enthalpy change of system ( Δ H s y s ) to absolute temperature ( T ). Δ S surr = − Δ H ° rxn T Explanation a. Δ H rxn º = – 385 kJ ; 298 K To estimate it, substitute the value of Δ H r x n º and the temperature in Kelvin in the equation Δ S surr = − Δ H rxn º T Δ S surr = − Δ H rxn º T = − 385 kJ 298 K = 1.29 × 10 3 J/K Hence, the change in entropy of the surrounding is 1.29 × 10 3 J/K . b. Δ H rxn º = – 385 kJ ; 77 K To calculate it, substitute the value of Δ H r x n ∘ and the temperature in Kelvin in the equation Δ S surr = − Δ H rxn ∘ T Δ S surr = − Δ H rxn ∘ T = − 385 kJ 77 K = 5.00 × 10 3 J/K c. Hence, the change in entropy of the surrounding is 5.00 × 10 3 J/K

Chemistry: A Molecular Approach (4th Edition)

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ISBN: 9780134112831

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 18, Problem 39E

Interpretation Introduction

Introduction: The entropy change of surroundings (ΔSsurr ) is negative of the ratio of enthalpy change of system (ΔHsys ) to absolute temperature (T).

ΔSsurr=−ΔH°rxnT

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Chapter 18, Problem 38E

Chapter 18, Problem 40E

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Part 3: AHm,system Mass of 1.00 M HCI Vol. of 1.00 M HCI Mass of NaOH(s) Total Mass in Calorimeter Mole product if HCI limiting reactant Trial 1 62.4009 1.511g Mole product if NaOH limiting reactant Limiting reactant Initial Temperature Final Temperature 23.8°C 37.6°C Change in Temperature AHm,system (calculated) Average AHm,system (calculated) (calculated) (calculated) Trial 2 64.006g 1.9599 (calculated) (calculated) (calculated) (calculated) (calculated) (calculated) 24.7°C 41.9°C (calculated) (calculated) (2 pts. each)

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Chapter 18 Solutions

Chemistry: A Molecular Approach (4th Edition)

Ch. 18 - Prob. 1SAQ Ch. 18 - Prob. 2SAQ Ch. 18 - Q3. Arrange the gases—F2, Ar, and CH3F—in order of...Ch. 18 - Q4. Calculate the change in entropy that occurs in...Ch. 18 - Q5. A reaction has a ΔHrxn = 54.2 kJ. Calculate...Ch. 18 - Prob. 6SAQ Ch. 18 - Q7. Use standard entropies to calculate for the...Ch. 18 - Q8. Use standard free energies of formation to...Ch. 18 - Q9. Find ΔG$$ for the reaction 2 A + B → 2 C from...Ch. 18 - Prob. 10SAQ

Ch. 18 - Prob. 11SAQ Ch. 18 - Prob. 12SAQ Ch. 18 - Prob. 13SAQ Ch. 18 - Prob. 14SAQ Ch. 18 - Prob. 15SAQ Ch. 18 - Prob. 16SAQ Ch. 18 - 1. What is the first law of thermodynamics, and...Ch. 18 - Prob. 2E Ch. 18 - 3. What is a perpetual motion machine? Can such a...Ch. 18 - 4. Is it more efficient to heat your home with a...Ch. 18 - 5. What is a spontaneous process? Provide an...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 - Prob. 15E Ch. 18 - 16. Predict the spontaneity of a reaction (and the...Ch. 18 - 17. State the third law of thermodynamics and...Ch. 18 - 18. Why is the standard entropy of a substance in...Ch. 18 - Prob. 19E Ch. 18 - Prob. 20E Ch. 18 - 21. What are three different methods to calculate...Ch. 18 - Prob. 22E Ch. 18 - Prob. 23E Ch. 18 - Prob. 24E Ch. 18 - Prob. 25E Ch. 18 - Prob. 26E Ch. 18 - 27. Which of these processes is spontaneous? a....Ch. 18 - 28. Which of these processes are nonspontaneous?...Ch. 18 - 29. Two systems, each composed of two particles...Ch. 18 - 30. Two systems, each composed of three particles...Ch. 18 - 31. Calculate the change in entropy that occurs in...Ch. 18 - 32. Calculate the change in entropy that occurs in...Ch. 18 - 33. Calculate the change in entropy that occurs in...Ch. 18 - 34. Calculate the change in entropy that occurs in...Ch. 18 - 35. Without doing any calculations, determine the...Ch. 18 - 36. Without doing any calculations, determine the...Ch. 18 - Prob. 37E Ch. 18 - 38. Without doing any calculations, determine the...Ch. 18 - 39. Calculate ΔSsurr at the indicated temperature...Ch. 18 - Prob. 40E Ch. 18 - 41. Given the values of ΔH$$, ΔS$$, and T,...Ch. 18 - Prob. 42E Ch. 18 - 43. Calculate the change in Gibbs free energy for...Ch. 18 - 44. Calculate the change in Gibbs free energy for...Ch. 18 - 45. Calculate the free energy change for this...Ch. 18 - Prob. 46E Ch. 18 - Prob. 47E Ch. 18 - Prob. 48E Ch. 18 - Prob. 49E Ch. 18 - 50. What is the molar entropy of a pure crystal at...Ch. 18 - Prob. 51E Ch. 18 - 52. For each pair of substances, choose the one...Ch. 18 - 53. Rank each set of substances in order of...Ch. 18 - 54. Rank each set of substances in order of...Ch. 18 - Prob. 55E 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. For each reaction, calculate , , and at 25 °C...Ch. 18 - 63. Use standard free energies of formation to...Ch. 18 - 64. Use standard free energies of formation to...Ch. 18 - 65. Consider the reaction: 2 NO(g) + O2(g) → 2...Ch. 18 - Prob. 66E Ch. 18 - 67. Determine ΔG° for the reaction: Fe2O3(s) + 3...Ch. 18 - 68. Calculate for the reaction: CaCO3(s) → CaO(s)...Ch. 18 - 69. Consider the sublimation of iodine at 25.0 °C...Ch. 18 - 70. Consider the evaporation of methanol at 25.0...Ch. 18 - 71. Consider the reaction: CH3OH(g) CO(g) + 2...Ch. 18 - Prob. 72E Ch. 18 - Prob. 73E Ch. 18 - Prob. 74E Ch. 18 - Prob. 75E Ch. 18 - Prob. 76E Ch. 18 - 77. Estimate the value of the equilibrium constant...Ch. 18 - 78. Estimate the value of the equilibrium constant...Ch. 18 - 79. Consider the reaction: H2(g) + I2(g) 2...Ch. 18 - Prob. 80E Ch. 18 - 81. The change in enthalpy () for a reaction is...Ch. 18 - Prob. 82E Ch. 18 - 83. Determine the sign of ΔSsys for each...Ch. 18 - 84. Determine the sign of ΔSsys for each...Ch. 18 - 85. Our atmosphere is composed primarily of...Ch. 18 - Prob. 86E Ch. 18 - 87. Ethene (C2H4) can be halogenated by the...Ch. 18 - 88. H2 reacts with the halogens (X2) according to...Ch. 18 - 89. Consider this reaction occurring at 298...Ch. 18 - 90. Consider this reaction occurring at 298...Ch. 18 - Prob. 91E Ch. 18 - Prob. 92E Ch. 18 - 93. These reactions are important in catalytic...Ch. 18 - Prob. 94E Ch. 18 - Prob. 95E Ch. 18 - Prob. 96E Ch. 18 - 97. Consider the reaction X2(g) → 2 X(g). When a...Ch. 18 - 98. Dinitrogen tetroxide decomposes to nitrogen...Ch. 18 - 99. Indicate and explain the sign of ΔSuniv for...Ch. 18 - Prob. 100E Ch. 18 - Prob. 101E Ch. 18 - Prob. 102E Ch. 18 - Prob. 103E Ch. 18 - Prob. 104E Ch. 18 - Prob. 105E Ch. 18 - Prob. 106E Ch. 18 - Prob. 107E Ch. 18 - 108. The salt ammonium nitrate can follow three...Ch. 18 - 109. Given the data, calculate ΔSvap for each of...Ch. 18 - Prob. 110E Ch. 18 - Prob. 111E Ch. 18 - Prob. 112E Ch. 18 - Prob. 113E Ch. 18 - 114. Which statement is true? a. A reaction in...Ch. 18 - Prob. 115E Ch. 18 - Prob. 116E Ch. 18 - Prob. 117E Ch. 18 - Prob. 118QGW Ch. 18 - Prob. 119QGW Ch. 18 - 120. Not all processes in which the system...Ch. 18 - Prob. 121QGW Ch. 18 - Prob. 122QGW Ch. 18 - Prob. 123DIA

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The entropy change of surroundings ( Δ S s u r r ) is negative of the ratio of enthalpy change of system ( Δ H s y s ) to absolute temperature ( T ). Δ S surr = − Δ H ° rxn T

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Introduction: The entropy change of surroundings (ΔSsurr ) is negative of the ratio of enthalpy change of system (ΔHsys ) to absolute temperature (T). ΔSsurr=−ΔH°rxnT

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Chapter 18 Solutions

Introduction: The entropy change of surroundings (ΔSsurr ) is negative of the ratio of enthalpy change of system (ΔHsys ) to absolute temperature (T).

ΔSsurr=−ΔH°rxnT