To calculate the final temperature after thermal equilibrium is reached, we need to consider the heat exchange between the two pieces of bismuth. We can start by using the heat equation:
ΔQ = mcΔT
where ΔQ is the heat exchange, m is the mass, c is the heat capacity, and ΔT is the change in temperature.
We can first calculate the heat absorbed by the solid bismuth, which is given by:
ΔQ1 = mc1ΔT1 = (27.7 g)(26.3 J K–1 mol–1)(253 °C - Tf)
where Tf is the final temperature.
Next, we can calculate the heat released by the liquid bismuth, which is given by:
ΔQ2 = -mc2ΔT2 = -(277 g)(31.6 J K–1 mol–1)(Tf - 333 °C)
Since the two pieces of bismuth are in thermal equilibrium, the heat absorbed by the solid must be equal to the heat released by the liquid, so we can set ΔQ1 = ΔQ2:
(27.7 g)(26.3 J K–1 mol–1)(253 °C - Tf) = -(277 g)(31.6 J K–1 mol–1)(Tf - 333 °C)
Solving for Tf, we find:
Tf = (253 °C - 333 °C)(27.7 g)(26.3 J K–1 mol–1) / [(277 g)(31.6 J K–1 mol–1)] + 333 °C
Tf = 324.4 °C
So the final temperature after thermal equilibrium is reached is 324.4 °C.