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The first law of thermodynamics for a cl...

The first law of thermodynamics for a closed system is dU = dq + dw, where dw = `dw_(pv)+dw_("non-pv")`. The most common type of `w_("non-pv")` is electrical work. As per IUPAC convention work done on the system is positive.
A system generates 50 J electrical energy, has 150 J of pressure-volume work done on it by the surroundings while releasing 300 J of heat energy. What is the change in the internal energy of the sytem?

A

`-500`

B

`-100`

C

`-300`

D

`-200`

Text Solution

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The correct Answer is:
To solve the problem, we will use the first law of thermodynamics, which states: \[ dU = dq + dw \] Where: - \( dU \) is the change in internal energy. - \( dq \) is the heat added to the system. - \( dw \) is the work done on the system. In this case, we can break down the work done into two components: - \( dw_{(pv)} \): Pressure-volume work done on the system. - \( dw_{(non-pv)} \): Non-pressure-volume work, which in this case is electrical work. ### Given Data: 1. Electrical energy generated (non-pv work) = 50 J (This is work done by the system, so it will be negative) 2. Pressure-volume work done on the system = 150 J (This is work done on the system, so it will be positive) 3. Heat energy released = 300 J (Since heat is released, it will be negative) ### Step-by-Step Solution: 1. **Identify the heat transfer (dq)**: \[ dq = -300 \, \text{J} \quad (\text{heat is released}) \] 2. **Identify the work done (dw)**: - Pressure-volume work done on the system: \[ dw_{(pv)} = +150 \, \text{J} \quad (\text{work done on the system is positive}) \] - Electrical work done by the system: \[ dw_{(non-pv)} = -50 \, \text{J} \quad (\text{work done by the system is negative}) \] 3. **Calculate total work done (dw)**: \[ dw = dw_{(pv)} + dw_{(non-pv)} = 150 \, \text{J} - 50 \, \text{J} = 100 \, \text{J} \] 4. **Apply the first law of thermodynamics**: \[ dU = dq + dw \] Substituting the values: \[ dU = -300 \, \text{J} + 100 \, \text{J} = -200 \, \text{J} \] 5. **Final Result**: The change in internal energy of the system is: \[ dU = -200 \, \text{J} \] ### Summary: The change in internal energy of the system is \(-200 \, \text{J}\). ---

To solve the problem, we will use the first law of thermodynamics, which states: \[ dU = dq + dw \] Where: - \( dU \) is the change in internal energy. - \( dq \) is the heat added to the system. - \( dw \) is the work done on the system. ...
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