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If DeltaG is negative, the reaction will...

If `DeltaG` is negative, the reaction will be

A

At equilibrium

B

Not possible

C

Both (a) and (b)

D

Possible

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To determine the nature of a reaction based on the value of Gibbs free energy change (ΔG), we can follow these steps: ### Step-by-Step Solution: 1. **Understanding ΔG**: The Gibbs free energy change (ΔG) is a thermodynamic quantity that helps predict the spontaneity of a reaction. It combines the enthalpy and entropy of a system. 2. **Evaluating ΔG Values**: - If ΔG > 0: The reaction is **non-spontaneous**. This means that the reaction will not occur under standard conditions. - If ΔG = 0: The reaction is at **equilibrium**. This indicates that the forward and reverse reactions occur at the same rate, and there is no net change in the concentrations of reactants and products. - If ΔG < 0: The reaction is **spontaneous**. This means that the reaction can occur without any external input of energy. 3. **Applying the Given Condition**: In the question, it is stated that ΔG is negative (ΔG < 0). According to the evaluation above, this indicates that the reaction is spontaneous. 4. **Conclusion**: Since ΔG is negative, we conclude that the reaction is spontaneous. ### Final Answer: If ΔG is negative, the reaction will be **spontaneous**. ---
To determine the nature of a reaction based on the value of Gibbs free energy change (ΔG), we can follow these steps: ### Step-by-Step Solution: 1. **Understanding ΔG**: The Gibbs free energy change (ΔG) is a thermodynamic quantity that helps predict the spontaneity of a reaction. It combines the enthalpy and entropy of a system. 2. **Evaluating ΔG Values**: - If ΔG > 0: The reaction is **non-spontaneous**. This means that the reaction will not occur under standard conditions. ...
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