Question

What would the final temperature of the pan and water be in Example 1.7 if 0.260 kg of water were placed in the pan and 0.0100 kg of the water evaporated immediately, leaving the remainder to come to a common temperature with the pan?

a) 45.8°C
b) 52.3°C
c) 60.7°C
d) 68.2°C

Answer 1

To find the final temperature after mixing water and a pan at different temperatures, the concept of calorimetry is used, based on the conservation of energy. Heat lost by the pan must equal the heat gained by the water, with adjustments for any water that evaporates. Exact calculations require additional information not provided in the question.

Step-by-step explanation:

To calculate the final temperature when mixing water with different masses at different temperatures, we must consider the heat exchange process between the two bodies, the water and the pan. In this case, we're dealing with calorimetry, a branch of thermodynamics that measures the heat of chemical reactions or physical changes. Using the principle of conservation of energy, the heat gained by the water as it warms up to the final temperature must be equal to the heat lost by the pan as it cools down to the same final temperature.

However, since there is an additional factor of 0.0100 kg of water evaporating immediately, this will affect the amount of heat required to achieve thermal equilibrium. The amount of heat needed to evaporate the water must be considered. Unfortunately, without more specific information, such as initial temperatures, heat capacities, or the heat of vaporization, a precise temperature cannot be calculated. If example Example 1.7 or the provided information contains this data, you would use these values to set up and solve the equation for the final temperature. The answer would depend on including those factors in the heat exchange equation.