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For a reaction at standard conditions, if ΔG° is positive, what does it indicate
For a reaction at standard conditions, if ΔG° is positive, what does it indicate?
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Practice Questions
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Q1
For a reaction at standard conditions, if ΔG° is positive, what does it indicate?
The reaction is spontaneous in the forward direction.
The reaction is non-spontaneous in the forward direction.
The reaction is at equilibrium.
The reaction is spontaneous in the reverse direction.
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A positive ΔG° indicates that the reaction is non-spontaneous in the forward direction.
Questions & Step-by-step Solutions
1 item
Q
Q: For a reaction at standard conditions, if ΔG° is positive, what does it indicate?
Solution:
A positive ΔG° indicates that the reaction is non-spontaneous in the forward direction.
Steps: 4
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 if a reaction has a positive ΔG°, it means that the reaction does not occur spontaneously in the forward direction.
Step 4: Conclude that a positive ΔG° suggests that the reaction will require energy input to proceed.
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