Problem:  531 cal of heat is added to 5.00 g ice at -20.0°C. What is the final temperature of the water?

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We’re being asked to determine the final temperature when 531 cal of heat is added to 5.00 g ice at -20.0°C.


The heat added will be absorbed by the iceWe’re going to calculate the final temperature using the following steps:

Step 1: Calculate the heat required in raising the temperature of 5.00 g of ice from -20.0°C to 0.0°C (q1). If the amount is less than the added heat, proceed to  to Step 2
Step 2: Calculate the heat required to melt 5.00 g of ice to 5.00 g of water at 0°C (q2). If the amount is less than the added heat, proceed to Step 3.
Step 3: Calculate the heat required in raising the temperature of 5.00 g of water from 00.0°C to the final temperature 100°C (q3). If the amount is greater than the added heat, proceed to Step 4.
Step 4: Calculate the final temperature (Tf).


Note that calorie (cal) is just another unit of energy similar to Joules (J) and 1 cal = 4.184 J. Convert 531 cal to J:

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Problem Details

 531 cal of heat is added to 5.00 g ice at -20.0°C. What is the final temperature of the water?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Heating and Cooling Curves concept. You can view video lessons to learn Heating and Cooling Curves. Or if you need more Heating and Cooling Curves practice, you can also practice Heating and Cooling Curves practice problems.