The transfer of 100 kJ of heat to a large mass of water at 0 o C (273 K) results

Question

The transfer of 100 kJ of heat to a large mass of water at 0 oC (273 K) results in a change of entropy of +366 J K-1, whereas the same heat transfer at 100 oC (373 K) results in a change of entropy of +268 J K-1.

Is the following statement true of false?

The definition of entropy implies that the process is more irreversible at a lower temperature, regardless of the fact that the amount of heat transferred is the same.

False

True

There is not enough information to decide on the correctness of the statement

False

True

There is not enough information to decide on the correctness of the statement

Explanation / Answer

Chanage in entropy (J/k)= Change in heat of system/ Temperature

Heat transferred = 100 kJ

Temperature = 0'C

Entropy = 100 x1000 J/273 K = 366.3004 J/K

Heat transferred = 100 kJ

Temperature = 100'C

Entropy = 100 x1000 J/373 K = 268.09 J/K

When heat is tranferred to a object which is already having some heat will have less impact then adding same quantity of heat to object at lower temperature.

It is like pouring hot water in a bucket of hot water and pouring same quantity of hot water with same temperature in to bucket of cold water.

the answer is true - Since in an irreversible process of adding heat from higher object to lower object entropy increases.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.