A beaker containing water at 373 K is representig an open system, is placed in the room. Predict the nature of work done.

Sure! Here are the step-by-step solutions: Given: The system does work on the surroundings and loses heat to the surroundings. We know that the work done by a system can be expressed as: $W=-P_{ext}\Delta V$ where $P_{ext}$ is the external pressure and $\Delta V$ is the change in volume of the system. We are told that the system does work on the surroundings, which means that the volume of the system changes. Since the work done by the system is negative, we can conclude that the volume of the system decreases. Therefore, we can rewrite the equation for work as: $W=-P_{ext}(-\Delta V)=P_{ext}\Delta V_{sys}$ where $\Delta V_{sys}$ is the change in volume of the system. We are also told that the system loses heat to the surroundings. According to the First Law of Thermodynamics, the change in internal energy of a system ($\Delta U$) is equal to the heat added to the system ($Q$) minus the work done by the system ($W$): $\Delta U=Q-W$ If the system loses heat to the surroundings, then $Q$ is negative. Therefore, we can rewrite the equation for the First Law as: $\Delta U=-|Q|-P_{ext}\Delta V_{sys}$ This means that the change in internal energy of the system is negative. In other words, the system is losing energy as it does work on the surroundings and loses heat to the surroundings.