Question

A 46.7 gram sample of Copper at 96.5°C is dropped into 85.1 g of cool water at 24.3°C. The water containing the Copper warms up to 27.7°C. How many calories does the metal lose?

Answer 1

The copper loses 289.34 calories when its temperature drops from 96.5°C to 27.7°C, based on the heat transfer to the water.

Step-by-step explanation:

To determine the calories the metal loses, we can use the concept of heat transfer. In an isolated system, heat lost by the hot substance is equal to the heat gained by the cool substance. The specific heat capacity of copper is 0.092 cal/g°C, and for water is 1 cal/g°C.

First, calculate the heat gained by water:

q = mass × specific heat × ΔT = 85.1 g × 1 cal/g°C × (27.7°C - 24.3°C) = 85.1 cal × 3.4°C = 289.34 cal

Since the system is isolated, the heat lost by copper will be equal to the heat gained by the water:

Heat lost by copper = Heat gained by water = 289.34 cal

Therefore, the copper loses 289.34 calories.