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Chapter 6: Problem 33

If the internal energy of a thermodynamic system is increased by \(300 . \mathrm{J}\) while \(75 \mathrm{~J}\) of expansion work is done, how much heat was transferred and in which direction, to or from the system?

Short Answer

Expert verified
The heat transferred (Q) is \(375 J\) and it was transferred to the thermodynamic system.

Step by step solution

01

Write down the first law of thermodynamics

The first law of thermodynamics states that ΔU = Q - W. Here, ΔU is the change in internal energy, Q is the heat transferred, and W is the work done.
02

Plug in the given values

We are given ΔU = 300 J and W = 75 J. Plug these values into the equation: \(300 = Q - 75\)
03

Solve for Q

Now, we will solve the equation for Q, the heat transferred: \(Q = 300 + 75\) \(Q = 375 J\)
04

Determine the direction of heat transfer

Since Q is positive, we can conclude that 375 J of heat was transferred to the system. If Q was negative, then heat would be transferred from the system. So, 375 J of heat was transferred to the thermodynamic system.

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