Section 1
Energy Transfer
What is heat?
What is temperature?
How does temperature differ from heat?
What is the enthalpy of a substance?
Define molar heat capacity.
How does molar heat capacity differ from specific heat?
How is the Kelvin temperature scale different from the Celsius and Fahrenheit scales?
Calculate the molar heat capacity of diamond, given that 63 $\mathrm{J}$ were needed to heat a 1.2 $\mathrm{g}$ of diamond by $1.0 \times 10^{2} \mathrm{K}$ .
Use the molar heat capacity for aluminum from table 1 to calculate the amount ofenergy needed to raise the temperature of 260.5 $\mathrm{g}$ of aluminum from $0^{\circ} \mathrm{C}$ to $125^{\circ} \mathrm{C}$ .
Use the molar heat capacity for iron from table 1 to calculate the amount of energyneeded to raise the temperature of 260.5 $\mathrm{g}$ of iron from $0^{\circ} \mathrm{C}$ to $125^{\circ} \mathrm{C}$
A sample of aluminum chloride increased in temperature by 3.5 $\mathrm{K}$ when the sampleabsorbed $1.67 \times 10^{2} \mathrm{J}$ of energy. Calculate the number of moles of aluminum chloride in this sample. Use table 1.
Use table 1 to determine the final temperature when $2.5 \times 10^{2} \mathrm{J}$ of energy as heat is transferred to 0.20 mol of helium at 298 $\mathrm{K}$ .
Predict the final temperature when 1.2 $\mathrm{kJ}$ of energy as heat is transferred from $1.0 \times$$10^{2} \mathrm{mL}$ of water at 298 $\mathrm{K}$ .
Use Table 1 to determine the specific heat of silver.
Use Table 1 to determine the specific heat of sodium chloride.
Why is a temperature difference the same in Celsius and Kelvin?
Predict the molar heat capacities of $\mathrm{PbS}(s)$ and $\mathrm{Ag}_{2} \mathrm{S}(s) .$
Use table 1 to predict the molar heat capacity of $\mathrm{FeCl}_{3}(s)$
Use your answer from item 18 to predict the specific heat of $\mathrm{FeCl}_{3}(s)$