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In a spontaneous reaction, the free ener...

In a spontaneous reaction, the free energy of a system :

A

increases

B

decreases

C

remains unchanged

D

becomes equal to zero

Text Solution

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The correct Answer is:
To solve the question regarding the behavior of free energy in a spontaneous reaction, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Spontaneous Reactions**: - A spontaneous reaction is one that occurs naturally without needing to be driven by an external force. These reactions tend to release energy. 2. **Concept of Free Energy**: - Free energy (Gibbs free energy, G) is a thermodynamic potential that measures the maximum reversible work that can be performed by a thermodynamic system at constant temperature and pressure. 3. **Energy Changes in Spontaneous Reactions**: - In spontaneous reactions, the system tends to move towards a lower energy state. This means that the free energy of the system decreases as the reaction proceeds. 4. **Effect on Surroundings**: - When a spontaneous reaction occurs, it often releases energy to the surroundings, which can lead to an increase in the free energy of the surroundings. However, this does not affect the free energy of the system itself. 5. **Conclusion**: - Therefore, in a spontaneous reaction, the free energy of the system decreases. 6. **Final Answer**: - The correct option is **B) decreases**.
To solve the question regarding the behavior of free energy in a spontaneous reaction, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Spontaneous Reactions**: - A spontaneous reaction is one that occurs naturally without needing to be driven by an external force. These reactions tend to release energy. 2. **Concept of Free Energy**: ...
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A chemical process always proceeds in the direction in which the Gibbs free energy of the system decreases.

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A change in the free energy of a system at constant temperature and pressure will be: Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S At constant temperature and pressure Delta_(sys) G lt 0 (spontaneous) Delta_(sys)G = 0 (equilibrium) Delta_(sys)G gt 0 (non-spontaneous) The free enegry for a reaction having DeltaH = 31400 cal, DeltaS = 32 cal K^(-1) mol^(-1) at 1000^(@)C is

A change in the free energy of a system at constant temperature and pressure will be: Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S At constant temperature and pressure Delta_(sys) G lt 0 (spontaneous) Delta_(sys)G = 0 (equilibrium) Delta_(sys)G gt 0 (non-spontaneous) For a spontaneous reaction DeltaG , equilibrium K and E_(cell)^(Theta) will be, respectively

A change in the free energy of a system at constant temperature and pressure will be: Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S At constant temperature and pressure Delta_(sys) G lt 0 (spontaneous) Delta_(sys)G = 0 (equilibrium) Delta_(sys)G gt 0 (non-spontaneous) If both DeltaH and Deltas are negative, the reaction will be spontaneous

Assertion :- Entropy of system increases for a spontaneous reactions. Reason :- Enthalpy of reaction always decreases for spontaneous reaction.