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For a reaction at standard conditions, if ΔG° is positive, what does it imply?
For a reaction at standard conditions, if ΔG° is positive, what does it imply?
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Practice Questions
1 question
Q1
For a reaction at standard conditions, if ΔG° is positive, what does it imply?
The reaction is spontaneous in the forward direction.
The reaction is at equilibrium.
The reaction is non-spontaneous in the forward direction.
The reaction will proceed rapidly.
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A positive ΔG° indicates that the reaction is non-spontaneous in the forward direction under standard conditions.
Questions & Step-by-step Solutions
1 item
Q
Q: For a reaction at standard conditions, if ΔG° is positive, what does it imply?
Solution:
A positive ΔG° indicates that the reaction is non-spontaneous in the forward direction under standard conditions.
Steps: 5
Show Steps
Step 1: Understand what ΔG° means. ΔG° is the change in Gibbs free energy for a reaction at standard conditions.
Step 2: Recognize that a positive ΔG° value indicates that the energy of the products is higher than the energy of the reactants.
Step 3: Know that a reaction is considered spontaneous if it can occur without external energy input.
Step 4: Since ΔG° is positive, it means the reaction does not occur naturally in the forward direction under standard conditions.
Step 5: Conclude that a positive ΔG° implies the reaction is non-spontaneous in the forward direction.
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