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Chapter 16
General Chemistry 2 Spring Semester 2026
| Question | Answer |
|---|---|
| Energy definition | The capacity to do work |
| Work definition | The result of a force acting over a distance |
| Heat definition | The flow of thermal energy caused by a temperature difference |
| Enthalpy definition | The sum of the internal energy and the product of pressure and volume (state function) |
| State function definition | Its value depends only on the state of the system, not on how the system arrived at that state |
| First law of thermodynamics | The energy of the universe is constant Energy is neither created not destroyed, but can be transferred from one object to another, and converted from one form to another |
| System definition | The material or process within which we are investigating the energy changes |
| Surrounding definition | Everything else with which the system can exchange energy |
| When does a spontaneous process occur? | Without the input of energy from outside the system |
| When does a non spontaneous process occur? | When energy is input to the system from outside the system Needs continuous input of energy |
| Does a spontaneous process have to happen quickly? | No, a spontaneous process does not have to be fast |
| What is entropy (S) ? | The measure of the randomness or disorder of a system |
| When S final is greater than S initial, what happens to the change in S and the randomness | Randomness is increased delta S is greater than 0 |
| When S final is less than S initial, what happens to the change in S and the randomness | Randomness is decreased delta S is less than 0 |
| Order the entropy of a solid, liquid, and a gas from ordered to disorderly | Solid < liquid < gas |
| When does entropy increase? | With the number of energetically equivalent ways to arrange components |
| What the the entropy equation | S = klnW k: the Boltzmann constant, 1.38 x 10^-23 W: the number of energetically equivalent ways to arrange the components (micro states) |
| As the number of micro states increases what happens to the reaction? | It becomes more disorderly and S increases |
| What causes S to increase? | Phase changes The number of moles of gas in a reaction increases then the delta S > 0 Temperature changes Molar mass Molecular complexity dissolving a sold Dissolving a gas |
| What happens to S as temperature increases? | S increases |
| What happens to S as molar mass incrases | S increases |
| What happens to S as molecules become more complex | S increases |
| What happens as a solid dissolves | S increases |
| What happens as a gas dissolves | S decrases |
| Second law of thermodynamics | For any spontaneous process, the entropy of the universe increases |
| What kind of a function is entropy? | State function |
| If the reaction is spontaneous the delta S of the universe is | Greater than 0 |
| If the reaction is non spontaneous the delta S of the universe is | Less than 0 |
| If the reaction is at equilibrium the delta S of the universe is | Equal to 0 |
| In which way does a chemical system proceed related to entropy? | A chemical system proceeds in a direction that increases the entropy of the universe |
| The more disorder | The higher the entropy |
| The more oder | The lower the entropy |
| The change in entropy of the surroundings is | proportional to the opposite change in the heat of the system Inversely proportional to the temperature at which the heat is transferred |
| Third law of thermodynamics | The entropy of a perfect crystal at absolute zero (0 K) is zero |
| Gibbs free energy (G) | A thermodynamic state function related to enthalpy (H) and entropy (S) |
| G is what? | The maximum amount of work energy that can be released to the surroundings at constant T and P |
| What is G also called | Chemical potential |
| When delta G of the system is < 0 the reaction is.... | Spontanteous |
| When delta G of the system is > 0 the reaction is.... | Non spontanteous |
| When delta G of the system is = 0 the reaction is.... | At equilibrium |
| When delta S is <0 there are ... | fewer micro states (order) |
| When delta S is >0 there are ... | more micro states (disorder) |
| When delat H of the reaction is < 0 the reaction is... | Exothermic |
| When delat H of the reaction is > 0 the reaction is... | Endothermic |
| Standard state definition | The state of a material at a defined set of conditions |
| The standard state for a gas | Pure gas at exactly 1 atm pressure |
| The standard state for a liquid or solid | Pure substance in its most stable form at exactly 1 atm pressure and temperature of interest (usually 25 degrees C) |
| The standard state for a substance in solution | Concentration exactly 1 M |
| Standard molar entropy (S^o) | The entropy of one mole of the substance under standard state |
| ∆𝑮^o𝒓𝒙n | The change in free energy between the products and the reactants for a chemical reaction at standard states |
| What are the three methods to calculate ∆𝑮^o𝒓𝒙n | Use tabulated delta H^o f and delta S^o Use tabulated free energy of formation Use ∆𝑮^o𝒓𝒙n of each step |
| Standard free energy of formation | The change in free energy when 1 mol of a compound in its standard state forms from its elements in their standard states |
| ∆𝑮^o f of most compounds is | negative |
| ∆𝑮^o f of elemenst in most stable allotrope is | zero |
Created by:
KristenR2025