Chemical Thermodynamics: Gibbs Free Energy quiz #1 Flashcards
Chemical Thermodynamics: Gibbs Free Energy quiz #1
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What does the sign of Gibbs Free Energy (ΔG) indicate about the spontaneity of a chemical reaction?
A negative ΔG indicates a spontaneous reaction, a positive ΔG indicates a non-spontaneous reaction, and ΔG equal to zero indicates the reaction is at equilibrium. How is Gibbs Free Energy (ΔG) related to the equilibrium constant (K) and the reaction quotient (Q)?
At equilibrium, ΔG = 0 and Q = K. For spontaneous reactions, ΔG < 0, K > 1, and Q < K. For non-spontaneous reactions, ΔG > 0, K < 1, and Q > K. Why is Gibbs Free Energy more useful than enthalpy (ΔH) or entropy (ΔS) alone for predicting reaction spontaneity?
Gibbs Free Energy combines both enthalpy and entropy changes, allowing for a more complete prediction of spontaneity under specific conditions, whereas ΔH and ΔS alone do not account for both energy and disorder. What is the equation for calculating Gibbs Free Energy under non-standard conditions?
ΔG = ΔG° + RT ln Q, where ΔG° is the standard Gibbs Free Energy change, R is the gas constant, T is temperature in Kelvin, and Q is the reaction quotient. What are the standard conditions for calculating standard Gibbs Free Energy (ΔG°)?
Standard conditions are 1 atmosphere pressure, 1 molar concentration, and a temperature of 25°C (298 K). What does a negative value of Gibbs Free Energy (ΔG) indicate about a chemical reaction?
A negative ΔG indicates the reaction is spontaneous and can occur without outside energy input. How are the values of ΔG, K, and Q related at equilibrium?
At equilibrium, ΔG = 0, the equilibrium constant K = 1, and the reaction quotient Q = K. Why is Gibbs Free Energy (ΔG) a better predictor of reaction spontaneity than enthalpy (ΔH) or entropy (ΔS) alone?
Gibbs Free Energy combines both enthalpy and entropy changes, providing a more complete prediction of spontaneity under specific conditions. What is the equation for calculating Gibbs Free Energy under non-standard conditions?
ΔG = ΔG° + RT ln Q, where ΔG° is the standard Gibbs Free Energy change, R is the gas constant, T is temperature in Kelvin, and Q is the reaction quotient. What are the standard conditions used when calculating standard Gibbs Free Energy (ΔG°)?
Standard conditions are 1 atmosphere pressure, 1 molar concentration, and a temperature of 25°C (298 K).
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