In the previous problem, how much more heat must be gained to raise the temperature of the melted ice to room temperature of 23 C
this is physics not math
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To find out how much more heat must be gained to raise the temperature of the melted ice to room temperature (23°C), we need to know the mass of the melted ice and the specific heat capacity of water.
1. Determine the mass of the melted ice: This information must be given in the problem statement. Let's assume the mass of the melted ice is 100 grams.
2. Determine the specific heat capacity of water: The specific heat capacity of a substance tells us how much heat energy is required to raise the temperature of a certain amount of that substance by a certain amount. The specific heat capacity of water is approximately 4.186 joules/gram°C.
3. Determine the temperature change: The starting temperature of the melted ice is 0°C, and we want to raise it to 23°C. Therefore, the temperature change is 23°C - 0°C = 23°C.
4. Use the formula Q = mcΔT to calculate the heat energy required:
- Q represents the heat energy (in joules)
- m represents the mass of the substance (in grams)
- c represents the specific heat capacity of the substance (in joules/gram°C)
- ΔT represents the temperature change (in °C)
In this case, Q = (100g) × (4.186 joules/gram°C) × (23°C - 0°C)
Solving the equation yields:
Q = 100g × 4.186 joules/gram°C × 23°C
Q = 9657.8 joules
Therefore, approximately 9657.8 joules of heat energy must be gained to raise the temperature of the melted ice to room temperature (23°C).