Question

A ‑ 25.5 ‑ g aluminum block is warmed to 65.4 ° C and plunged into an insulated beaker containing 55.2 g water initially at 22.2 ° C . The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?

Answer 1

To determine the final temperature of a system consisting of two metal samples and water when they reach thermal equilibrium, we can use the principle of conservation of energy.

Step-by-step explanation:

In this problem, we are given the initial temperature of two metal samples and water, and we need to determine the final temperature of the system when they reach thermal equilibrium. To solve this problem, we can use the principle of conservation of energy.

We need to calculate the heat gained or lost by each component and set them equal to each other since no heat is lost to the surroundings.

Using the specific heat capacity formula Q = mcΔT, where Q is the heat gained or lost, m is the mass, c is the specific heat capacity, and ΔT is the temperature change, we can calculate the final temperature of the system.