A sample of steam with a mass of 0.552 g and at a temperature of 100 °C condenses into an insulated container holding 4.25 g of water at 5.0 °C. Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture?

Key Concepts

Heat Transfer and Conservation of Energy

In thermodynamics, the principle of conservation of energy states that energy cannot be created or destroyed, only transformed. In this scenario, the heat lost by the steam as it condenses and cools must equal the heat gained by the water as it warms up. This relationship allows us to set up an equation to solve for the final temperature of the mixture.

Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise the temperature of a unit mass of a substance by one degree Celsius. Different substances have different specific heat capacities, which affect how they respond to heat transfer. In this problem, the specific heat capacities of steam and water will be crucial for calculating the heat exchange during the condensation and warming processes.

Phase Change and Latent Heat

Phase changes, such as the condensation of steam into water, involve latent heat, which is the heat absorbed or released during a phase transition without a change in temperature. The latent heat of vaporization for water is significant in this problem, as it quantifies the energy released when steam condenses. Understanding this concept is essential for accurately calculating the heat transfer involved in the process.