DrBob222. when you move ice from zero to final T. Do you add 100 cal.?
To determine if you need to add 100 calories when moving ice from 0°C to the final temperature, you need to consider the specific heat and any phase changes involved.
First, let's assume we are dealing with ice at 0°C and want to raise its temperature to a final temperature T.
1. Calculate the heat required to raise the temperature of ice:
The specific heat capacity of ice is 2.09 J/g°C (joules per gram per degree Celsius). To convert this to calories, divide by 4.18 (since 1 calorie = 4.18 joules).
So, the specific heat capacity of ice is approximately 0.50 cal/g°C.
To calculate the heat required to raise the temperature, use the formula:
Heat (cal) = Mass (g) * Specific heat capacity (cal/g°C) * Temperature change (°C)
2. Determine the mass of the ice:
You need to know the mass of the ice you are working with. This can be measured or given in the problem statement.
3. Calculate the heat required to raise the temperature to the final temperature:
Multiply the mass of the ice by the specific heat capacity of ice and the temperature change (final temperature - 0°C). This value will give you the amount of heat required to raise the temperature of the ice.
If the final temperature T is greater than 0°C, T > 0°C, then you will need to add heat to the ice to raise its temperature. In this case, you can use the calculated heat value as the answer.
However, if the final temperature T is below 0°C, T < 0°C, then you can ignore the heat calculation because the ice will remain in a solid state at a temperature below its melting point of 0°C. In this case, no heat needs to be added.
In summary, whether you need to add 100 calories or not depends on the final temperature T. If T > 0°C, you need to calculate and add the heat required. If T < 0°C, then no heat needs to be added since the ice remains in a solid state.