Question

If a 50.0 g ball of iron at 160.0 °C is dropped into 50.0 g of water at 20.0°C in an insulated container, what will be the final temperature of the water? The specific heat of iron is 0.444 g•°C, and that of water is 4.18 J/g degrees Celsius.

A) 20.0 °C
B) 30.0 °C
C) 40.0 °C
D) 50.0 °C

Answer 1

The final temperature of the water after the iron ball is dropped into it will be 30.0 °C.

Step-by-step explanation:

To find the final temperature of the water, we can use the principle of conservation of energy. The heat lost by the iron ball will be equal to the heat gained by the water.

First, we calculate the heat lost by the iron ball using the equation: Q = m * c * ∆T, where Q is the heat lost, m is the mass, c is the specific heat capacity, and ∆T is the change in temperature.

Next, we calculate the heat gained by the water using the same equation, substituting the specific heat capacity of water and the initial and final temperatures.

Finally, we can equate the two amounts of heat and solve for the final temperature of the water.

In this case, the final temperature of the water after the iron ball is dropped into it will be B) 30.0 °C.