A certain system absorbs 0.300 kJ of heat and has 0.700 kJ of work performed on it. What is th

step 1 So for Q here, this is going to be positive 0 .300 kilojoules. And it's positive. As we're told,

A certain system absorbs 0.300 kJ of heat and has 0.700 kJ...

A certain system absorbs $0.300 \mathrm{~kJ}$ of heat and has $0.700 \mathrm{~kJ}$ of work performed on it. What is the value of $\Delta E$ for the change? Is the overall change exothermic or endothermic?

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Key Concepts

Endothermic and Exothermic Processes

Processes are classified as endothermic or exothermic based on the direction of heat transfer. An endothermic process, characterized by a positive Q, occurs when a system absorbs heat from its surroundings, while an exothermic process involves the system releasing heat. Distinguishing between these processes helps in determining the nature of the energy changes occurring within the system.

First Law of Thermodynamics

This law states that the energy of an isolated system is conserved. It is typically expressed as ?E = Q + W, where ?E is the change in internal energy, Q is the heat added to the system, and W is the work done on the system. Understanding this principle is foundational in thermodynamics, as it explains how energy transfers affect the system's internal energy.

Sign Conventions in Thermodynamics

In thermodynamics, the proper application of sign conventions is critical. When heat is absorbed by the system, Q is taken as positive, indicating an increase in internal energy due to heat intake. Similarly, when work is done on the system, W is positive, meaning that this work contributes positively to the system's internal energy. These conventions are necessary for correctly applying the first law of thermodynamics.

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