Introductory Chemistry (6th Edition)
6th Edition
ISBN: 9780134302386
Author: Nivaldo J. Tro
Publisher: PEARSON
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Chapter 12, Problem 5SAQ
Interpretation Introduction
Interpretation: The first point on a graph where a sample of ice, which is heated past its melting point, contains no solid ice is to be determined.
Concept Introduction: Melting point of a substance is defined as the state at which the solid and liquid is in equilibrium with each other. It depends on the types of intermolecular forces present in a molecule. Stronger intermolecular force results in higher value of melting point.
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What property of water explains why water inside the tiny cracks in rocks helps the latter break when it freezes?
a. Water has a high boiling point
b. Water has a high surface tension
c. Water has a greater volume in its solid state
d. Water has a high heat of vaporization
A pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. Here is a
graph of the results:
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5 kJ/mol of heat has been added?
Submit
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gas
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A solid substance melts at 15 °C. Which is true for the same substance?
This substance in its liquid form will boil at 15 °C.
This substance in its gas form will vaporize at 15 °C.
This substance in its liquid form will freeze at 15 °C.
This substance in its gas form will condense at 15 °C.
Chapter 12 Solutions
Introductory Chemistry (6th Edition)
Ch. 12 - The first diagram shown here represents liquid...Ch. 12 - Prob. 2SAQCh. 12 - Prob. 3SAQCh. 12 - How many 20.0-g ice cubes are required to absorb...Ch. 12 - Prob. 5SAQCh. 12 - Prob. 6SAQCh. 12 - Prob. 7SAQCh. 12 - Prob. 8SAQCh. 12 - Prob. 9SAQCh. 12 - Prob. 10SAQ
Ch. 12 - Prob. 1ECh. 12 - Prob. 2ECh. 12 - What determines whether a substance is a solid,...Ch. 12 - 4. What are the properties of liquids? Explain the...Ch. 12 - 5. What are the properties of solids? Explain the...Ch. 12 - Prob. 6ECh. 12 - Prob. 7ECh. 12 - Prob. 8ECh. 12 - Prob. 9ECh. 12 - Why does a glass of water evaporate more slowly in...Ch. 12 - Prob. 11ECh. 12 - Prob. 12ECh. 12 - 13. Acetone evaporates more quickly than water at...Ch. 12 - Prob. 14ECh. 12 - Prob. 15ECh. 12 - Prob. 16ECh. 12 - 17. Explain why a steam burn from gaseous water at...Ch. 12 - Prob. 18ECh. 12 - Prob. 19ECh. 12 - Prob. 20ECh. 12 - Is the melting of ice endothermic or exothermic?...Ch. 12 - 22. Is the boiling of water endothermic or...Ch. 12 - Prob. 23ECh. 12 - Prob. 24ECh. 12 - 25. What is hydrogen bonding? How can you tell...Ch. 12 - Prob. 26ECh. 12 - Prob. 27ECh. 12 - Prob. 28ECh. 12 - Prob. 29ECh. 12 - Prob. 30ECh. 12 - Prob. 31ECh. 12 - 32. What is an atomic solid? What are the...Ch. 12 - Prob. 33ECh. 12 - Prob. 34ECh. 12 - Prob. 35ECh. 12 - Two samples of pure water of equal volume are put...Ch. 12 - Prob. 37ECh. 12 - Spilling water over your skin on a hot day will...Ch. 12 - Prob. 39ECh. 12 - Water is put into a beaker and heated with a...Ch. 12 - 41. Which causes a more severe burn: spilling 0.50...Ch. 12 - 42. The nightly winter temperature drop in a...Ch. 12 - Prob. 43ECh. 12 - Prob. 44ECh. 12 - 45. An ice chest is filled with 3.5 kg of ice at...Ch. 12 - Why does 50 g of water initially at 0 C warm more...Ch. 12 - In Denver, Colorado, water boils at 95. C....Ch. 12 - Prob. 48ECh. 12 - 49. How much heat is required to vaporize 33.8 g...Ch. 12 - How much heat is required to vaporize 43.9 g of...Ch. 12 - How much heat does your body lose when 2.8 g of...Ch. 12 - How much heat does your body lose when 4.86 g of...Ch. 12 - How much heat is emitted when 4.25 g of water...Ch. 12 - Prob. 54ECh. 12 - 55. The human body obtains 835 kJ of energy from a...Ch. 12 - 56. The human body obtains 1078 kJ from a candy...Ch. 12 - How much heat is required to melt 37.4 g of ice at...Ch. 12 - 58. How much heat is required to melt 23.9 g of...Ch. 12 - How much energy is released when 34.2 g of water...Ch. 12 - How much energy is released when 2.55 kg of...Ch. 12 - 61. How much heat is required to convert 2.55 g of...Ch. 12 - 62. How much heat is required to convert 5.88 g of...Ch. 12 - Prob. 63ECh. 12 - Prob. 64ECh. 12 - 65. What kinds of intermolecular forces are...Ch. 12 - Prob. 66ECh. 12 - Prob. 67ECh. 12 - What kinds of intermolecular forces are present in...Ch. 12 - Which substance has the highest boiling point?...Ch. 12 - Prob. 70ECh. 12 - One of these two substances is a liquid at room...Ch. 12 - Prob. 72ECh. 12 - 73. A flask containing a mixture of and is...Ch. 12 - 74. Explain why is a liquid at room temperature...Ch. 12 - Are CH3CH2CH2CH2CH3 and H2O miscible?Ch. 12 - Prob. 76ECh. 12 - Prob. 77ECh. 12 - 78. Determine whether a homogeneous solution forms...Ch. 12 - 79. Identify each solid as molecular, ionic, or...Ch. 12 - Prob. 80ECh. 12 - Identify each solid as molecular, ionic, or...Ch. 12 - Identify each solid as molecular, ionic, or...Ch. 12 - 83. Which solid has the highest melting point?...Ch. 12 - 84. Which solid has the highest melting point?...Ch. 12 - 85. For each pair of solids, determine which solid...Ch. 12 - For each pair of solids, determine which solid has...Ch. 12 - 87. List these substances in order of increasing...Ch. 12 - 88. List these substances in order of decreasing...Ch. 12 - 89. Ice actually has negative caloric content. How...Ch. 12 - Prob. 90ECh. 12 - An 8.5-g ice cube is placed into 255 g of water....Ch. 12 - A 14.7-g ice cube is placed into 324 g of water....Ch. 12 - 93. How much ice in grams would have to melt to...Ch. 12 - Prob. 94ECh. 12 - Prob. 95ECh. 12 - Prob. 96ECh. 12 - Draw a Lewis structure for each molecule and...Ch. 12 - Draw a Lewis structure for each molecule and...Ch. 12 - 99. The melting point of ionic solids depends on...Ch. 12 - Draw ionic Lewis structures for KF and CaO. Use...Ch. 12 - Prob. 101ECh. 12 - Prob. 102ECh. 12 - An ice cube at 0.00 C with a mass of 23.5 g is...Ch. 12 - Prob. 104ECh. 12 - Prob. 105ECh. 12 - Prob. 106ECh. 12 - Prob. 107ECh. 12 - Prob. 108ECh. 12 - Prob. 109QGWCh. 12 - Prob. 110QGWCh. 12 - Prob. 111QGWCh. 12 - Prob. 112QGWCh. 12 - Prob. 113DIA
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- A pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. A graph of the results is shown in the picture. A. Using the graph, what is the melting point of X? B. What phase (physical state) of X would you expect to find in the flask after 9 kJ/mol of heat has been added? Select all that apply: solid, liquid, or gasarrow_forwardUse the observation in the first column to answer the question in the second column. observation question Which has a higher vapor pressure? At 1 atm pressure, Substance E Substance E boils at -11. °C and Substance F Substance F boils at 11. °C. Neither, E and F have the same vapor pressure. It's impossible to know without more information. Which has the higher boiling point? Substance C The enthalpy of vaporization of Substance C is bigger than Substance D that of Substance D. Neither, C and D have the same boiling point. It's impossible to know without more information. Which has a higher enthalpy of vaporization? At 22 °C, Substance A has a Substance A vapor pressure of 125. torr and Substance B has a vapor Substance B pressure of 155. torr. Neither, A and B have the same enthalpy of vaporization. It's impossible to know without more information.arrow_forwardA pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. Here is a graph of the results: 180. 160. temperature (°C) 140. 120. 100. 0. 10. What is the melting point of X ? Use this graph to answer the following questions: heat added (kJ/mol) What phase (physical state) of X would you expect to find in the flask after 20 kJ/mol of heat has been added? 20. ооо °C 30. (check all that apply) solid liquid gas 40.arrow_forward
- A pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. Here is a graph of the results: temperature (°C) 160. 140. 120. 100. 80. 0. 10. What is the melting point of X ? Use this graph to answer the following questions: heat added (kJ/mol) What phase (physical state) of X would you expect to find in the flask after 18 kJ/mol of heat has been added? 20. 000 30. 11°C (check all that apply) solid liquid gas 40.arrow_forwardPart A. Use these facts on the heating and cooling curve of water in answering the following activities. Direction: Analyze each of the following statements whether it describes the heating and cooling curve of water. Write TRUE if the statement is correct but if it’s false, change the underlined word or group of words to make the whole statement true. Write your answer on a separate sheet of paper. 3. The melting point of a solid and freezing point of a liquid is the temperature where the solid and liquid phase of water co-exist at equilibrium.arrow_forwardIce floats on water. For most other substances, however, the solid sinks in the liquid. Classify each of these statements based on whether they describe water or most other substances. Water Most other substances nswer Bank The molecules are closest in the liquid phase. High pressure will cause the liquid to become solid. The molecules are closest in the solid phase. The solid is less dense than the liquid. The solid is more dense than the liquid. In a phase diagram, the solid-liquid coexistence line has a negative slope. In a phase diagram, the solid-liquid coexistence line has a positive slope. High pressure will cause the solid to become liquid.arrow_forward
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