Exactly 10 mL of water at 25°C was added to a hot iron skillet. All of the water was converted into steam at 100°C. If the mass of the pan was 1.20 kg and the molar heat capacity of iron is 25.19 J/mol∙°C, what was the temperature change of the skillet?

Answer 1

The temperature change of the skillet can be calculated using the equation for the heat capacity of a substance, which is $q=mc\Delta T$, where $q$ is the heat, $m$ is the mass, $c$ is the specific heat capacity, and $\Delta T$ is the temperature change.

In this case, the heat absorbed by the skillet is the heat of vaporization of water, which is 40.7 kJ/mol. Since the skillet has a mass of 1.20 kg and the molar heat capacity of iron is 25.19 J/mol∙°C, the temperature change can be calculated as follows:

$\Delta T = \frac{q}{mc} = \frac{40.7 \text{ kJ/mol}}{1.20 \text{ kg} \cdot 25.19 \text{ J/mol∙°C}} = 1.61 \text{ °C}$

Therefore, the temperature of the skillet increased by 1.61°C when the water was added.