Question

1. a system absorbs 196 kj of heat and the surroundings of 117 kj of work on the system. what is the change in internal energy of the system?

Explanation:

Step1: Recall the first - law formula

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

Step2: Identify the values of $Q$ and $W$

The system absorbs heat, so $Q = 196\ kJ$ (positive because heat is added to the system). The surroundings do work on the system, so $W=117\ kJ$ (positive because work is done on the system).

Step3: Calculate $\Delta U$

Substitute $Q = 196\ kJ$ and $W = 117\ kJ$ into the formula $\Delta U=Q + W$. Then $\Delta U=196\ kJ+117\ kJ$.
$\Delta U = 313\ kJ$

Answer:

$313\ kJ$