Answer
During this vaporization process, 11300 J of heat were absorbed.
Work Step by Step
1. Identify the objective.
- Find the number of joules that are necessary to vaporize 5.00 g of water at 100$^{\circ}$.
2. Find the conversion factors.
- To convert the mass in g to joules in a vaporization process, we can use the Heat of Vaporization for water.
Page 79: $\frac{2260J}{1g}$ and $\frac{1g}{2260J}$
3. Using the conversion factor, calculate the necessary heat:
$5.00 g \times \times \frac{2260 J}{1g} = 11300 J$
4. Adjust the number to the correct number of significant figures.
- The used number that has the fewest number of significant figures is "5.00", with 3. Therefore, the result of the multiplication must have 3 SFs.
11300 J = 11300 J
5. Indicate whether heat was absorbed or released.
- During the vaporization process, heat is absorbed.
