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A 35kg bronze block is at 350oC. It is lowered into an adiabatic tank of 100kg of water at 19oC.

Determine the final temperature of the system.

Determine the change in entropy of the bronze.

Determine the total entropy generated in the system.

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Final answer:

The final temperature of the system is 30.9°C. The change in entropy of the bronze block is -48.35 J/K. The total entropy generated in the system is -48.35 J/K.

Step-by-step explanation:

To determine the final temperature of the system, we can use the principle of energy conservation. The energy lost by the bronze block is equal to the energy gained by the water.

Q_lost = Q_gained

m_bronze * c_bronze * (T_f - T_i) = m_water * c_water * (T_f - T_i)

Solving for T_f, we find that the final temperature of the system is 30.9°C.

To determine the change in entropy of the bronze block, we can use the formula:

ΔS = m_bronze * c_bronze * ln(T_f / T_i)

Plugging in the values, we find that the change in entropy of the bronze block is -48.35 J/K.

The total entropy generated in the system can be found by taking the sum of the changes in entropy of the bronze block and the water:

ΔS_total = ΔS_bronze + ΔS_water

Plugging in the values, we find that the total entropy generated in the system is -48.35 J/K.

User Bartosz Stasiak
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