(c) Assume that a chunk of potassium weighing 7.55 g is dropped into 400.0 g of water at 25.0 °C. What is the final temperature of the water if all the heat released is used to warm the water?

Key Concepts

Heat Transfer

Heat transfer is the process by which thermal energy moves from one object or substance to another due to a temperature difference. In this scenario, the heat released by the potassium as it reacts with water will be absorbed by the water, leading to an increase in its temperature. Understanding this concept is crucial for calculating the final temperature of the water.

Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. Each substance has a unique specific heat capacity, which influences how much its temperature will change when heat is added or removed. For water, the specific heat capacity is approximately 4.18 J/g°C, which is essential for determining how much the temperature of the water will increase in response to the heat from the potassium.

Calorimetry

Calorimetry is the science of measuring the heat of chemical reactions or physical changes. In this problem, calorimetry principles can be applied to calculate the final temperature of the water by equating the heat lost by the potassium to the heat gained by the water. This involves using the formula Q = mcΔT, where Q is the heat exchanged, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.