AP Chemistry thermodynamics concepts such as enthalpy, entropy, and free energy, plus electrochemistry including redox and galvanic cells.
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- Define enthalpy
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The heat energy of a system, equal to the internal energy plus the product of pressure and volume (H = U + PV)- Define entropy
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A measure of disorder or the number of possible arrangements of particles in a system- What is Gibbs free energy?
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The maximum useful work a system can perform at constant temperature and pressure, calculated as ΔG = ΔH - TΔS- A reaction is spontaneous at all temperatures when
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ΔH is negative and ΔS is positive (ΔG is always negative)- An exothermic reaction is one where
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Energy is released to the surroundings, so ΔH is negative- An endothermic reaction is one where
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Energy is absorbed from the surroundings, so ΔH is positive- Define heat capacity
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The amount of heat energy required to raise the temperature of a substance by one degree- State Hess's Law
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The enthalpy change of a reaction is the same regardless of the pathway taken, depending only on initial and final states- What is standard enthalpy of formation?
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The enthalpy change when one mole of a compound is formed from its elements in their standard states- Entropy increases when a system
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Becomes more disordered or dispersed, as occurs during phase changes from solid to liquid to gas, or dissolution, or mixing- ____ equals zero at equilibrium
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ΔG- At high temperatures, an endothermic reaction with positive entropy change becomes
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Spontaneous, because the TΔS term dominates the ΔH - TΔS equation- Define oxidation
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Loss of electrons or an increase in oxidation state- Define reduction
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Gain of electrons or a decrease in oxidation state- What is the oxidation state of oxygen in most compounds?
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Minus 2, except in peroxides where it is minus 1 and in OF2 where it is plus 2
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