Question

1. the gas in a cylinder (defined as the system) warms and absorbs 655 j of heat. the expansion performs 344 j of work on the surroundings. what is the change in internal energy for the system?

Explanation:

Step1: Recall the first law of thermodynamics

The first law of thermodynamics is given by $\Delta U = Q - W$, where $\Delta U$ is the change in internal energy, $Q$ is the heat added to the system, and $W$ is the work done by the system.

Step2: Substitute the given values

Here, $Q = 655\ J$ (heat absorbed by the system, so positive) and $W=344\ J$ (work done by the system, so positive).
Substitute these values into the formula: $\Delta U=655 - 344$.

Step3: Calculate the result

$\Delta U = 655-344=311\ J$.

Answer:

The change in internal energy for the system is $311\ J$.