How Do You Calculate Temperature Changes and Heat Requirements in Water?

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To calculate the temperature drop of 1.00 kg of water losing 83.8 kJ of heat, the result is a decrease of 0.2 degrees Celsius using the specific heat capacity of water. For raising the temperature of 10.0 kg of water by 20.0 degrees Celsius, the heat required can be determined by applying the specific heat formula, factoring in the mass and temperature change. The specific heat capacity of water is 4.19 J/g°C, which must be adjusted for the larger mass of 10,000 grams. The discussion emphasizes the importance of using the correct equations for these calculations. Understanding these principles is crucial for accurate thermal energy assessments in water.
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1. How many celsius degrees does the temperature of a mass of 1.00 kg of water fall for each 83.8 kJ of heat it loses.
2. Not so sure about EQUATIONS but I have my own way of going at it.
3. 83.8 kJ / 4.19 J * (1.00 kg * 1000) = 0.2 degrees celsius



1. How much heat is required to raise the temperature of a mass of 10.0 kg of water a total of 20.0 celsius degrees.
2. Not so sure about EQUATIONS but I have my own way of going at it.
3. IF it takes 4.19 j of heat to raise the temperature of 1 gram of water by one degree celsius, how do we factor in the larger mass of 10,000 grams and the larger temperature change of 20 celsius degrees?
 
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Your solution to the first question is correct. For the second, you should consider an equation relating the specific heat capacity of water, its mass and the change in temperature to thermal energy. I'm sure you will have been given some formulae in your notes/text.
 
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