Introductory Chemistry: A Foundation
9th Edition
ISBN: 9781337399425
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
Chapter 14, Problem 19ALQ
Interpretation Introduction
Interpretation:
Why it is incorrect to use molecule of
Concept Introduction:
Substance in which discrete molecules are present in that case molecules of the substance is present.
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provide the balanced equation: the reaction of zinc metal with sulfuric acid (H2SO4) solution produces bubbles on the surface of the zinc metal.
Consider the melting points of the substances below (see figures for two compounds). Explain the trend in melting point using your knowledge of intermolecular forces. (In the structures below, carbon is black, hydrogen is white, and oxygen is red.)
Substance
Melting Point (°C)
Molar Mass (g/mol)
Cl2
−102
71
Ethyl formate (CH3CH2OCHO)
−80
74
Propionic acid (CH3CH2COOH)
−20
74
Br2
−7.2
160
Based on the kinetic molecular model, solids usually have higher densities compare two liquids. However, ice , a solid form of H2O floats on liquid water which means ice is less dense than water. What do you think is the reason for this phenomenon? What is the biological significance of this concept?
Chapter 14 Solutions
Introductory Chemistry: A Foundation
Ch. 14.2 - trong>Exercise 14.1 Calculate the total energy...Ch. 14.3 - Prob. 1CTCh. 14.6 - trong>Exercise 14.2 Name the type of crystalline...Ch. 14 - ou seal a container half-filled with water. Which...Ch. 14 - xplain the following: You add 100mLof water to a...Ch. 14 - Prob. 3ALQCh. 14 - Prob. 4ALQCh. 14 - Prob. 5ALQCh. 14 - Prob. 6ALQCh. 14 - Prob. 7ALQ
Ch. 14 - ow do the following physical properties depend on...Ch. 14 - ook at Fig. 14.2. Why doesn't temperature increase...Ch. 14 - Prob. 10ALQCh. 14 - Prob. 11ALQCh. 14 - Prob. 12ALQCh. 14 - Prob. 13ALQCh. 14 - Prob. 14ALQCh. 14 - Prob. 15ALQCh. 14 - True or false? Methane (CH4) is more likely In...Ch. 14 - Prob. 17ALQCh. 14 - Prob. 18ALQCh. 14 - Prob. 19ALQCh. 14 - Which would you predict should be larger for a...Ch. 14 - Prob. 21ALQCh. 14 - Prob. 22ALQCh. 14 - Prob. 23ALQCh. 14 - ases have (higher/lower) densities than liquids or...Ch. 14 - Prob. 2QAPCh. 14 - Prob. 3QAPCh. 14 - he enthalpy (H)of vaporization of water is about...Ch. 14 - Prob. 5QAPCh. 14 - Prob. 6QAPCh. 14 - Prob. 7QAPCh. 14 - Prob. 8QAPCh. 14 - Prob. 9QAPCh. 14 - Prob. 10QAPCh. 14 - Prob. 11QAPCh. 14 - The energy required to melt 1 mole of a solid is...Ch. 14 - The following data have ban collected for...Ch. 14 - The molar heat of fusion of aluminum metal is...Ch. 14 - Prob. 15QAPCh. 14 - Prob. 16QAPCh. 14 - The molar heats of fusion and vaporization for...Ch. 14 - It requires 113Jto melt 1.00gof sodium metal at...Ch. 14 - Consider the iodine monochloride molecule, ICI....Ch. 14 - Prob. 20QAPCh. 14 - Prob. 21QAPCh. 14 - Prob. 22QAPCh. 14 - Prob. 23QAPCh. 14 - Prob. 24QAPCh. 14 - What type of intermolecular forces is active in...Ch. 14 - Prob. 26QAPCh. 14 - Prob. 27QAPCh. 14 - The heats of fusion of three substances are listed...Ch. 14 - When dry ammonia gas (NH3)is bubbled into a...Ch. 14 - Prob. 30QAPCh. 14 - Prob. 31QAPCh. 14 - If you've ever opened a bottle of rubbing alcohol...Ch. 14 - Prob. 33QAPCh. 14 - Prob. 34QAPCh. 14 - Which substance in each pair would be expected to...Ch. 14 - Which substance in each pair would be expected to...Ch. 14 - Prob. 37QAPCh. 14 - Two molecules that contain the same number of each...Ch. 14 - Prob. 39QAPCh. 14 - Prob. 40QAPCh. 14 - How do ionic solids differ in structure from...Ch. 14 - A common prank on college campuses is to switch...Ch. 14 - Prob. 43QAPCh. 14 - What types of forces exist between the individual...Ch. 14 - Prob. 45QAPCh. 14 - Prob. 46QAPCh. 14 - Prob. 47QAPCh. 14 - Prob. 48QAPCh. 14 - Prob. 49QAPCh. 14 - Prob. 50QAPCh. 14 - Prob. 51APCh. 14 - Prob. 52APCh. 14 - Prob. 53APCh. 14 - Prob. 54APCh. 14 - Prob. 55APCh. 14 - Prob. 56APCh. 14 - Prob. 57APCh. 14 - Prob. 58APCh. 14 - Prob. 59APCh. 14 - Prob. 60APCh. 14 - Given the densities and conditions of ice, liquid...Ch. 14 - Prob. 62APCh. 14 - Which of the substances in each of the following...Ch. 14 - Prob. 64APCh. 14 - Prob. 65APCh. 14 - Prob. 66APCh. 14 - Prob. 67APCh. 14 - Prob. 68APCh. 14 - Describe, on both a microscopic and a macroscopic...Ch. 14 - Cake mixes and other packaged foods that require...Ch. 14 - Prob. 71APCh. 14 - Prob. 72APCh. 14 - The molar heat of vaporization of carbon...Ch. 14 - Prob. 74APCh. 14 - Prob. 75APCh. 14 - Prob. 76APCh. 14 - Prob. 77APCh. 14 - Prob. 78APCh. 14 - Prob. 79APCh. 14 - Prob. 80APCh. 14 - Prob. 81APCh. 14 - Prob. 82APCh. 14 - Prob. 83APCh. 14 - Prob. 84APCh. 14 - Describe in detail the microscopic processes that...Ch. 14 - Prob. 86APCh. 14 - Formaldehyde has the formula CH2O, where C is the...Ch. 14 - Prob. 88APCh. 14 - Prob. 89APCh. 14 - Describe, on a microscopic basis, the processes of...Ch. 14 - Prob. 91APCh. 14 - Prob. 92APCh. 14 - Which of the following compound(s) exhibit only...Ch. 14 - Which of the following statements about...Ch. 14 - Prob. 95CPCh. 14 - Prob. 96CPCh. 14 - Prob. 97CPCh. 14 - Which of the following statements is(are) true?...
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Similar questions
- 12)arrow_forward1. When a chunk of dry ice (solid carbon dioxide) is placed out in the air, the solid gradually disappears and a gas is formed above the solid. Does it go through chemical or physical change has occurred? Explain. 2. When the molecules of the solid CO2 becomes free upon exposure to the air. What happened to the bonds of the molecule?arrow_forwardThe graph in Figure 5 below shows the variation in melting and boiling points for the elements in Group IV of the Periodic Table. Melting and Boiling Points of Group 4 elements 5000 |MPt (°C) |BPt C) 4000 3000 2000 1000 0+ Si Ge Sn Pb Figure 5: Diagram showing the melting and boiling points for the elements in Group IV of the Periodic Table. Figure taken from www.bing.com; accessed 19 May 2021. a) What is the general trend observed in Figure 5? b) Explain the variation in the melting and boiling points of the element in Group IV of the Periodic Table, shown in Figure 5, in terms of structure and bonding. { 11 }arrow_forward
- Which of these two compounds has a higher melting point and why ?arrow_forwardDetermine the electronegativity difference and the molecular polarity (P for polar and NP for nonpolar) of the following compounds then further classify the dominant intermolecular forces of attraction exhibited. Place HB for hydrogen bonding, LDF for London dispersion force, DD for dipole-dipole and ID for the ion-dipole bond. The first one is already done for you. 1.78 | P | hydrogen fluoride | HB 02 C2H6 NH4 H2O I2 HFarrow_forwardNonearrow_forward
- Use vapor pressure. A student leaving campus for spring break wants to make sure the air in her dorm room has a high water vapor pressure so that her plants are comfortable. The dorm room measures 3.76 m × 4.17 m × 3.31 m and the student places a pan containing 1.62 L of water in the room. Assume that the room is airtight, that there is no water vapor in the air when she closes the door, and that the temperature remains a constant 25 °C. The vapor pressure of water at 25 °C is 23.8 mm Hg. (a) Calculate the pressure that the water vapor would exert if all of the liquid water evaporated. mm Hg (b) Will all of the water in the pan evaporate?arrow_forwardPick a substance expected to have the lowest boiling point? O A. sodium nitrate, NaNO3 O B. diamond OC methane, CH4 OD. glycerine, C3H5(OH)3 O E. copperarrow_forwardThere are three sets of sketches below, showing the same pure molecular compound (ammonia, molecular formula NH,) at three different temperatures. The sketches are drawn as if a sample of ammonia were under a microscope so powerful that individual atoms could be seen. Only one sketch in each set is correct. Use the slider to choose the correct sketch in each set. You may need the following information: melting point of NH3: – 77.7 °C boiling point of NH3: – 33.3 °C 00 A (Choose one) (Choose one) (Choose one) do 4 5 4 5. 21. °C - 60. °C - 89. °C Tra JAN .. W 14 ... MacBook Air DII DD 80 000 000 F11 F7 F8 F9 F10 F1 F4 F5 F6 F2 F3arrow_forward
- According to one of the principles of combustion, solid and liquid fuels must be changed to a gas before they burn. For liquid fuels, this is easily explained as liquids vaporize when enough heat is applied to reach the boiling point. How can you explain the same principle of combustion with regards to solid fuels like coal?Answer in less than 100 words.arrow_forwardWhich of the following compounds has the highest melting point? Carbon dioxide, CO2 H2S Benzene, C6H6 H2O Sucrose, C12H22O11arrow_forwardUse vapor pressure. A student leaving campus for spring break wants to make sure the air in his dorm room has a high water vapor pressure so that his plants are comfortable. The dorm room measures 3.41 mx 4.41 m x 3.90 m and the student places a pan containing 0.874 L of water in the room. Assume that the room is airtight, that there is no water vapor in the air when he closes the door, and that the temperature remains a constant 22 °C. The vapor pressure of water at 22 °C is 19.8 mm Hg. (a) Calculate the pressure that the water vapor would exert if all of the liquid water evaporated. mm Hg (b) Will all of the water in the pan evaporate? [arrow_forward
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