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 ice. **We’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 (q_{1}). 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 (q_{2}). 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 (q_{3}). If the amount is greater than the added heat, proceed to Step 4.**Step 4****:** Calculate the final temperature (T_{f}).

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**:

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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