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Chapter 12: Problem 6

If amount of heat given to a system is \(50 \mathrm{~J}\) and work done on the system is \(15 \mathrm{~J}\), then change in internal energy of the system is (A) \(35 \mathrm{~J}\) (B) \(50 \mathrm{~J}\) (C) \(65 \mathrm{~J}\) (D) \(15 \mathrm{~J}\)

Short Answer

Expert verified
The change in internal energy of the system is \(35 \mathrm{~J}\).

Step by step solution

01

Identify the given values

In this problem, we are given the amount of heat given to the system (Q) as 50 J and the work done on the system (W) as 15 J.
02

Recall the First Law of Thermodynamics

The First Law of Thermodynamics states that "the change in the internal energy (鈭哢) of a system is equal to the heat added to the system (Q) minus the work done by the system (W)". Mathematically, this can be written as: \(鈭哢 = Q - W\)
03

Substitute the given values

Now, plug in the given values of Q and W into the formula: \(鈭哢 = 50 \mathrm{~J} - 15 \mathrm{~J}\)
04

Calculate the change in internal energy

Calculate the difference between the heat given to the system and the work done on the system: \(鈭哢 = 35 \mathrm{~J}\) So the correct answer is (A) \(\bold{35 \mathrm{~J}}\). The change in internal energy of the system is 35 J.

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Most popular questions from this chapter

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