If 25.00 ml of water is removed from two flasks, one with less water initially and each at 25 degrees, what will happen to the temp in each flask?
To determine what will happen to the temperature in each flask after removing 25.00 ml of water, we need to consider the principles of heat transfer and specific heat capacity.
Assuming that the flasks and the water inside them are initially at the same temperature (25 degrees Celsius), we can analyze the situation based on the following information:
1. Specific Heat Capacity: Different substances have different abilities to store heat energy. Water has a relatively high specific heat capacity, which means it can absorb or release a significant amount of heat energy without a large change in temperature.
2. Conservation of Energy: When heat is transferred between two objects, the total amount of heat energy remains constant. In this case, the total heat energy in the system (flasks + water) will remain the same, assuming no heat is gained or lost to the surroundings.
Now, let's examine the two flasks after removing 25.00 ml of water:
Flask 1 (initially with less water):
Since flask 1 has less water initially, removing 25.00 ml of water will have a relatively larger impact on the heat energy stored in the remaining water. Consequently, the temperature of the water in flask 1 will increase.
Flask 2 (initially with more water):
For flask 2, even with the removal of 25.00 ml of water, the remaining water volume is still relatively large. Thus, the impact on the heat energy stored in the water will be smaller compared to flask 1. As a result, the temperature of the water in flask 2 will experience a smaller increase compared to flask 1.
Therefore, after removing 25.00 ml of water, the temperature will increase more in the flask that initially had less water, while the temperature increase in the flask that initially had more water will be less pronounced.