A thermodynamic process occurs in which a system changes by -8 J/K. According to the second law of thermodynamics, what can you conclude about the entropy change of the environment? (a) it must be -8J/K or less (b) it must be equal to -8 J/K (c) it must be between -8J/K and zero (d) it must be zero (e) it must be between zero and +8J/K (f) it must be equal to +8J/K (g) it must be +8 J/K or more (h) we need to know the nature of the process to reach a conclusion (i) it is impossible for the system to have a negative entropy change.

The second law of thermodynamics says that any spontaneously occurring process always affects escalation in the entropy (S) of the universe. In simple words, according to this law, an isolated system's entropy never decreases over time.

The law itself mentions that the entropy of an isolated system can't decrease. This is because isolated systems spontaneously evolve towards thermodynamic equilibrium. So, the entropy of the environment will increase.

In some cases the system may be in thermodynamic equilibrium or may go through a reversible process, then the total entropy of a system and its surroundings will remains constant.

The correct answer is option (g) it must be +8J/k or more.

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