- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution142
- Ch.5 - Thermochemistry110
- Ch.6 - Electronic Structure of Atoms120
- Ch.7 - Periodic Properties of the Elements109
- Ch.8 - Basic Concepts of Chemical Bonding107
- Ch.9 - Molecular Geometry and Bonding Theories132
- Ch.10 - Gases132
- Ch.11 - Liquids and Intermolecular Forces74
- Ch.12 - Solids and Modern Materials87
- Ch.13 - Properties of Solutions85
- Ch.14 - Chemical Kinetics121
- Ch.15 - Chemical Equilibrium63
- Ch.16 - Acid-Base Equilibria104
- Ch.17 - Additional Aspects of Aqueous Equilibria105
- Ch.18 - Chemistry of the Environment52
- Ch.19 - Chemical Thermodynamics99
- Ch.20 - Electrochemistry103
- Ch.21 - Nuclear Chemistry64
- Ch.22 - Chemistry of the Nonmetals6
- Ch.23 - Transition Metals and Coordination Chemistry18
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Chapter 19, Problem 23a
The normal boiling point of Br2(l) is 58.8 °C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. (a) When Br2(l) boils at its normal boiling point, does its entropy increase or decrease?
Video transcript
The normal freezing point of n-octane (C8H18) is -57 °C. (d) Is there any temperature at which liquid n-octane and solid n-octane are in equilibrium? Explain.
A system goes from state 1 to state 2 and back to state 1 following a reversible path in both directions. Which of the following statements about this process is or are true?
c. The value of w on going from state 1 to state 2 is equal in magnitude and opposite in sign to the value of w on going from state 2 back to state 1.
Indicate whether each statement is true or false. (a) ΔS is a state function. (b) If a system undergoes a reversible change, the entropy of the universe increases. (c) If a system undergoes a reversible process, the change in entropy of the system is exactly matched by an equal and opposite change in the entropy of the surroundings. (d) If a system undergoes a reversible process, the entropy change of the system must be zero.
The normal boiling point of Br2(𝑙) is 58.8 °C, and its molar enthalpy of vaporization is Δ𝐻vap=29.6 kJ/mol. (b) Calculate the value of Δ𝑆 when 1.00 mol of Br2(𝑙) is vaporized at 58.8 °C.
The element gallium (Ga) freezes at 29.8 °C, and its molar enthalpy of fusion is ΔHfus = 5.59 kJ/mol. (a) When molten gallium solidifies to Ga(s) at its normal melting point, is ΔS positive or negative?
The element gallium (Ga) freezes at 29.8 °C, and its molar enthalpy of fusion is ΔHfus = 5.59 kJ/mol. (b) Calculate the value of ΔS when 60.0 g of Ga(l) solidifies at 29.8 °C.