A hot lump of 43.1 g of aluminum at an initial temperature of 55.2 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
[(mass Al x specific heat Al x (Tfinal-Tinitial)] + [(mass H2O x specific heat H2O x (Tfinal-Tinitial)]
mass Al is in the problem.
specific heat Al is in the problem.
Tf = solve for this
Ti for Al is in the problem.
mass H2O in the problem.
specific heat H2O = 4.18 J/*C
Tfinal = you're solving for this. It's in two places but that's just algebra.
Tinitial H2O = in the problem.
Post your work if you run into trouble.