Explanation Given information: Initial temperature = 80 ∘ C . Final temperature = 110 ∘ C . Δ H ( v a p o r i s a t i o n ) = 40.7 × 10 3 J / m o l . The heat capacity of water = 75.3 J / ( m o l K ) . The heat capacity of water vapor = 25.0 J / ( m o l K ) . The heat change required to raise the temperature of water from 80 ∘ C t o 100 ∘ C is calculated using q = m ( C w ) Δ T where m = Mass of water (g) = 18 g (1 mole). C w = heat capacity of water = 4.2 J/g/ ° C Δ T = change in temperature = ( 110 – 80 ) ∘ C = 20 ∘ C Thus, q = m ( C w ) Δ T = 18 × 4.2 × 30 = 1512 J = 1.512 kJ The heat needed to vaporize the water is determined using H 2 O ( l ) → H 2 O ( g ) ( 100 ∘ C ) Δ H ( v ) = q = 40.67 kJ The heat change needed to raise the temperature of vaporized water from 100 ∘ C t o 110 ∘ C requires the same equation as used before, but using a different heat capacity

Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition)

4th Edition

ISBN: 9780134162485

Author: Nivaldo J. Tro

Publisher: PEARSON

See similar textbooks

Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that …

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energ…

Videos

Question

Chapter 6, Problem 128E

Interpretation Introduction

To determine: q,w,ΔE, and ΔH for change in state of water.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 6, Problem 127E

Chapter 6, Problem 129E

Students have asked these similar questions

PLEASE HELP! URGENT!

"Water gas" is an industrial fuel composed of a mixture of carbon monoxide and hydrogen gases. When this fuel is burned, carbon dioxide and water result. From the information given below, write a balanced equation and determine the enthalpy of this reaction: CO(g) + O2(g) → CO₂(g) + 282.8 kJ H2(g) + O2(g) → H₂O(g) + 241.8 kJ MacBook Air

Page of 3 4. Calculate AG for the following reaction at 25°C. Will the reaction occur (be spontaneous)? How do you know? NH3(g) + HCl(g) → NH4Cl(s) AH=-176.0 kJ AS-284.8 J-K-1

Chapter 6 Solutions

Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition)

Ch. 6 - A chemical system produces 155 kJ of heat and does...Ch. 6 - Q2. Which sample is most likely to undergo the...Ch. 6 - Prob. 3SAQ Ch. 6 - Q4. A 12.5-g sample of granite initially at 82.0...Ch. 6 - Q5. A cylinder with a moving piston expands from...Ch. 6 - Prob. 6SAQ Ch. 6 - Q7. Hydrogen gas reacts with oxygen to form...Ch. 6 - Prob. 8SAQ Ch. 6 - Prob. 9SAQ Ch. 6 - Prob. 10SAQ

Ch. 6 - Prob. 11SAQ Ch. 6 - Prob. 12SAQ Ch. 6 - Prob. 13SAQ Ch. 6 - Prob. 14SAQ Ch. 6 - Q15. Natural gas burns in air to form carbon...Ch. 6 - 1. What is thermochemistry? Why is it important? Ch. 6 - 2. What is energy? What is work? List some...Ch. 6 - Prob. 3E Ch. 6 - 4. State the law of conservation of energy. How...Ch. 6 - Prob. 5E Ch. 6 - 6. State the first law of thermodynamics. What are...Ch. 6 - Prob. 7E Ch. 6 - 8. What is a state function? List some examples of...Ch. 6 - 9. What is internal energy? Is internal energy a...Ch. 6 - 10. If energy flows out of a chemical system and...Ch. 6 - 11. If the internal energy of the products of a...Ch. 6 - 12. What is heat? Explain the difference between...Ch. 6 - 13. How is the change in internal energy of a...Ch. 6 - 14. Explain how the sum of heat and work can be a...Ch. 6 - 15. What is heat capacity? Explain the difference...Ch. 6 - 16. Explain how the high specific heat capacity of...Ch. 6 - 17. If two objects, A and B, of different...Ch. 6 - 18. What is pressure–volume work? How is it...Ch. 6 - 19. What is calorimetry? Explain the difference...Ch. 6 - 20. What is the change in enthalpy (ΔH) for a...Ch. 6 - 21. Explain the difference between an exothermic...Ch. 6 - 22. From a molecular viewpoint, where does the...Ch. 6 - 23. From a molecular viewpoint, where does the...Ch. 6 - 24. Is the change in enthalpy for a reaction an...Ch. 6 - Prob. 25E Ch. 6 - Prob. 26E Ch. 6 - 27. What is a standard state? What is the standard...Ch. 6 - Prob. 28E Ch. 6 - 29. How do you calculate from tabulated standard...Ch. 6 - Prob. 30E Ch. 6 - 31. What are the main environmental problems...Ch. 6 - Prob. 32E Ch. 6 - Prob. 33E Ch. 6 - Prob. 34E Ch. 6 - Prob. 35E Ch. 6 - 36. A particular frost-free refrigerator uses...Ch. 6 - 37. Which statement is true of the internal energy...Ch. 6 - Prob. 38E Ch. 6 - 39. Identify each energy exchange as primarily...Ch. 6 - 40. Identify each energy exchange as primarily...Ch. 6 - 41. A system releases 622 kJ of heat and does 105...Ch. 6 - 42. A system absorbs 196 kJ of heat and the...Ch. 6 - 43. The gas in a piston (defined as the system)...Ch. 6 - Prob. 44E Ch. 6 - Prob. 45E Ch. 6 - Prob. 46E Ch. 6 - 47. How much heat is required to warm 1.50 L of...Ch. 6 - 48. How much heat is required to warm 1.50 kg of...Ch. 6 - 49. Suppose that 25 g of each substance is...Ch. 6 - 50. An unknown mass of each substance, initially...Ch. 6 - 51. How much work (in J) is required to expand the...Ch. 6 - Prob. 52E Ch. 6 - 53. The air within a piston equipped with a...Ch. 6 - 54. A gas is compressed from an initial volume of...Ch. 6 - 55. When 1 mol of a fuel burns at constant...Ch. 6 - 56. The change in internal energy for the...Ch. 6 - 57. Determine whether each process is exothermic...Ch. 6 - 58. Determine whether each process is exothermic...Ch. 6 - 59. Consider the thermochemical equation for the...Ch. 6 - 60. What mass of natural gas (CH4) must burn to...Ch. 6 - Prob. 61E Ch. 6 - Prob. 62E Ch. 6 - Prob. 63E Ch. 6 - Prob. 64E Ch. 6 - 65. A silver block, initially at 58.5 °C, is...Ch. 6 - Prob. 66E Ch. 6 - 67. A 31.1-g wafer of pure gold, initially at 69.3...Ch. 6 - Prob. 68E Ch. 6 - Prob. 69E Ch. 6 - 70. A 2.74-g sample of a substance suspected of...Ch. 6 - 71. Exactly 1.5 g of a fuel burns under conditions...Ch. 6 - 72. In order to obtain the largest possible amount...Ch. 6 - 73. When 0.514 g of biphenyl (C12H10) undergoes...Ch. 6 - Prob. 74E Ch. 6 - 75. Zinc metal reacts with hydrochloric acid...Ch. 6 - Prob. 76E Ch. 6 - 77. For each generic reaction, determine the value...Ch. 6 - Prob. 78E Ch. 6 - 79. Calculate ΔHrxn for the reaction: Fe2O3(s) + 3...Ch. 6 - 80. Calculate ΔHrxn for the reaction: CaO(s) +...Ch. 6 - 81. Calculate ΔHrxn for the reaction: 5 C(s) + 6...Ch. 6 - 82. Calculate ΔHrxn for the reaction: CH4(g) + 4...Ch. 6 - 83. Write an equation for the formation of each...Ch. 6 - Prob. 84E Ch. 6 - 85. Hydrazine (N2H4) is a fuel used by some...Ch. 6 - Prob. 86E Ch. 6 - Prob. 87E Ch. 6 - Prob. 88E Ch. 6 - 89. During photosynthesis, plants use energy from...Ch. 6 - Prob. 90E Ch. 6 - 91. Top fuel dragsters and funny cars burn...Ch. 6 - 92. The explosive nitroglycerin (C3H5N3O9)...Ch. 6 - 93. Determine the mass of CO2 produced by burning...Ch. 6 - Prob. 94E Ch. 6 - Prob. 95E Ch. 6 - Prob. 96E Ch. 6 - Prob. 97E Ch. 6 - Prob. 98E Ch. 6 - 99. Evaporating sweat cools the body because...Ch. 6 - Prob. 100E Ch. 6 - 101. Use standard enthalpies of formation to...Ch. 6 - 102. Dry ice is solid carbon dioxide. Instead of...Ch. 6 - 103. A 25.5-g aluminum block is warmed to 65.4 °C...Ch. 6 - Prob. 104E Ch. 6 - Prob. 105E Ch. 6 - Prob. 106E Ch. 6 - 107. Derive a relationship between ΔH and ΔE for a...Ch. 6 - Prob. 108E Ch. 6 - Prob. 109E Ch. 6 - Prob. 110E Ch. 6 - Prob. 111E Ch. 6 - 112. When 10.00 g of phosphorus is burned in O2(g)...Ch. 6 - Prob. 113E Ch. 6 - 114. The of TiI3(s) is –328 kJ/mol and the ΔH°...Ch. 6 - Prob. 115E Ch. 6 - Prob. 116E Ch. 6 - Prob. 117E Ch. 6 - 118. A pure gold ring and a pure silver ring have...Ch. 6 - Prob. 119E Ch. 6 - Prob. 120E Ch. 6 - Prob. 121E Ch. 6 - Prob. 122E Ch. 6 - Prob. 123E Ch. 6 - Prob. 124E Ch. 6 - Prob. 125E Ch. 6 - Prob. 126E Ch. 6 - Prob. 127E Ch. 6 - Prob. 128E Ch. 6 - Prob. 129E Ch. 6 - Prob. 130E Ch. 6 - 131. Which statement is true of the internal...Ch. 6 - Prob. 132E Ch. 6 - 133. Which expression describes the heat evolved...Ch. 6 - Prob. 134E Ch. 6 - 135. A 1-kg cylinder of aluminum and 1-kg jug of...Ch. 6 - Prob. 136E Ch. 6 - 137. When 1 mol of a gas burns at constant...Ch. 6 - Prob. 138E Ch. 6 - Prob. 139E Ch. 6 - Have each group member write a problem involving...Ch. 6 - Prob. 141QGW Ch. 6 - Prob. 142QGW Ch. 6 - Prob. 143QGW Ch. 6 - Prob. 144DIA

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

q , w , Δ E , and Δ H for change in state of water.

Concept explainers

Videos

To determine: q,w,ΔE, and ΔH for change in state of water.

Want to see the full answer?

Chapter 6 Solutions