Heat Effects and Calorimetry
A metal sample weighing \(147.90 \mathrm{g}\) and at a temperature of
\(99.5^{\circ} \mathrm{C}\) was placed in \(49.73 \mathrm{g}\) of water in a
calorimeter at \(23.0^{\circ} \mathrm{C}\). At equilibrium the temperature of
the water and metal was \(41.8^{\circ} \mathrm{C}\).
a. What was \(\Delta t\) for the water? \(\left(\Delta t=t_{\text {final
}}-t_{\text {intilial }}\right)\)
________ \(^{\circ} \mathrm{C}\)
b. What was \(\Delta t\) for the metal?
________\(^{\circ} \mathrm{C}\)
c. How much heat flowed into the water? (Take the specific heat of the water
to be 4.18 J/g \(^{\circ}\) C.)
_______ joules
d. Calculate the specific heat of the metal, using Equation 3.
______joules/g"C
e. What is the approximate molar mass of the metal? (Use Eq. 4.)
______\(g /m o l\)
