As temperature is increased above absolute zero, all materials undergo phase change: solid →liquid →gas Likewise, as temperature is decreased, all materials undergo phase change: gas → liquid →solid. At low temperatures, thermal energy promotes the low density (sold) state; at high temperatures, intermolecular attractive forces promote the random motion of molecules within the high density (gas) state ● At low temperatures, intermolecular attractive forces promote the high density (sold) state; at high temperatures, thermal energy promotes the random motion of molecules within the low density (gas) state At low temperatures, thermal energy promotes the high density (sold) state; at high temperatures, intermolecular attractive forces promote the random motion of molecules within the low density (gas) state At low temperatures, intermolecular attractive forces promote the low density (sold) state; at high temperatures, thermal energy promotes the random motion of molecules within the high density (gas) state

As temperature is increased above absolute zero, all materials undergo phase change: solid →liquid →gas Likewise, as temperature is decreased, all materials undergo phase change: gas → liquid →solid. At low temperatures, thermal energy promotes the low density (sold) state; at high temperatures, intermolecular attractive forces promote the random motion of molecules within the high density (gas) state ● At low temperatures, intermolecular attractive forces promote the high density (sold) state; at high temperatures, thermal energy promotes the random motion of molecules within the low density (gas) state At low temperatures, thermal energy promotes the high density (sold) state; at high temperatures, intermolecular attractive forces promote the random motion of molecules within the low density (gas) state At low temperatures, intermolecular attractive forces promote the low density (sold) state; at high temperatures, thermal energy promotes the random motion of molecules within the high density (gas) state

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A cube of solid benzene (C6H6; M = 78.11 g/mol) at its melting point and weighing 8.90 g is placed in 21.6 g of water at 39.0 °C. Given that the heat of fusion of benzene is 9.92 kJ/mol, to what temperature will the water have cooled by the time all of the benzene has melted. You can assume that the benzene remains at its melting point.
How much energy is required to heat 17.1 g acetone (MM = 58.08 g/mol) from a solid at -114.0°C to a liquid at -27.0°C? The following physical data may be useful.ΔHfus = 7.27 kJ/molSpecific Heat - liquid = 2.16 J/g°CSpecific Heat - Gas = 1.29 J/g°CSpecific Heat - Solid = 1.6
What amount of heat (in kJ) is required to convert 30.0 g of an unknown solid (MM = 67.44 g/mol) at -15.4 °C to a liquid at 42.7 °C? (specific heat capacity of solid = 1.95 J/g･°C; specific heat capacity of liquid = 1.18 J/g･°C; ∆Hfus = 5.72 kJ/mol; normal freezing point, Tf = 28.3°C)
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 3.25 m × 4.03 m × 3.04 m and the student places a pan containing 0.580 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 22 °C. The vapor pressure of water at 22 °C is 19.8 mm Hg. Calculate the pressure that the water vapor would exert if all of the liquid water evaporated. mm Hg Will all of the water in the pan evaporate?
What amount of heat (in kJ) is required to convert 19.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g-°C; specific heat capacity of liquid = 1.58 J/g-°C; AHfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)
Two 20.0 g ice cubes at -17.00C are placed into 470.1 g of water at 25.0 0C. The heat of fusion of ice is 6.008 kJ/mol, the molar heat capacity of water is 75.3 J mol-1 K-1 and the molar heat capacity of ice is 37.7 J mol-1 K-1. Assuming no energy is transferred to or from the surroundings, please calculate the final temperature of the water after all the ice melts. _______ 0C
What amount of heat (in kJ) is required to convert 15.5 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)
Liquid butane is used in cigarette lighters. The boiling point of butane at 1 atm pressure is -1.0 °C and its ∆H(vap) is 22.44 kJ/mol. R = 8.314 ×10⁻³ kJ/mol･K. Calculate the pressure (in atm) of the butane in the lighter at 19.5 °C.
Calculate the heat required to convert 22.2 g of propyl alcohol, C3H3O, from a solid at -141°C into the gaseous state at 115°C. The normal melting and boiling points of this substance are -127°C and 97°C, respectively. The heat of fusion is 86.2 J/g, and the heat of vaporization is 694 J/g. The specific heats of the solid, liquid and gaseous states are, respectively, 2.36, 2.83 and 1.76 J/g/K.
What amount of heat (in kJ) is required to convert 10.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･ °C; specific heat capacity of liquid = 1.58 J/g･ °C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3 °C)
What amount of heat (in kJ) is required to convert 10.8 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g. °C; specific heat capacity of gas = 0.932 J/g⋅ °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3 °C)