Heat of Fusion
Ice cubes at 0 °C with a mass of 26 g are added to your soft drink.
a. How much heat (cal) must be added to melt all the ice at 0 °C?
b. What happens to the temperature of your soft drink? Why?

Question

Accepted Answer

a. The heat in calories required to melt the ice is calculated as follows:
Step 1 List the grams of substance and change of state.
Given 26 g of [latex]\mathrm{H}_{2}O(s)[/latex] Need calories to melt ice
Step 2 Write the plan to convert grams to heat and desired unit.

[latex]\text{grams of ice} \begin{matrix}\text{Heat of} \ \text{fusion}\end{matrix} \text{calories}[/latex]

Step 3 Write the heat conversion factor and metric factor if needed.

[latex]1 g of \mathsf{\,H_{2}O(s \rightarrow l)= 80.cal}\[/latex]

[latex]\frac{80 . cal} {1 g H_{2}O } and \frac{1 g H_{2}O }{80 . cal}[/latex]

Step 4 Set up the problem with factors.

[latex]26 \cancel{g H_{2}O}\times \frac{80 . cal}{1 \cancel{g H_{2}O}} =2100 cal[/latex]

b. The soft drink will be colder because heat from the soft drink is providing the
energy to melt the ice.

Question 2.SP.9: Heat of Fusion Ice cubes at 0 °C with a mass of 26 g are add......

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