Answer
During this condensation process, 5400 cal of heat were released.
Work Step by Step
1. Identify the objective.
- Find the number of calories that are necessary to condense 10.0 g of steam at 100$^{\circ}$.
2. Find the conversion factors.
- To convert the mass in g to calories in a condensation process, we can use the Heat of Vaporization for water.
Page 79: $\frac{540cal}{1g}$ and $\frac{1g}{540cal}$
3. Using the conversion factor, calculate the necessary heat:
$10.0 g \times \times \frac{540cal}{1g} = 5400 cal$
4. Adjust the number to the correct number of significant figures.
- The used number that has the fewest number of significant figures is "540", with 2. Therefore, the result of the multiplication must have 2 SFs.
5400 cal = 5400 cal
5. Indicate whether heat was absorbed or released.
- During the condensation process, heat is released.
You can check this information on page 76.