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

###### FREE Expert Solution

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:

85% (338 ratings) ###### 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?