ΔG°, or standard Gibbs free energy change, is the difference in Gibbs free energy between the products and reactants under standard conditions (1 atm pressure and 298K). It predicts whether a reaction will be spontaneous or not.
Think of ΔG° as a mountain guide who tells you how difficult your hike will be. If the value is negative, it's like going downhill - easy and spontaneous. But if it's positive, you're hiking uphill - non-spontaneous and requires external energy.
Standard Conditions: These are set conditions under which scientific measurements are made, typically at 1 atmosphere of pressure and temperatures around 25 degrees Celsius (298K).
Spontaneity: In chemistry, spontaneity refers to a process that can occur without being driven by an outside force. A negative ΔG° indicates a spontaneous reaction.
Entropy (ΔS): This is the measure of disorder or randomness in a system. It plays a key role in determining Gibbs free energy.
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