(a) We place 119.5 g of a metal at 25.00 o C in 423.8 g of water at 95.00 o C. The water is in a beaker that is also at 95.00 o C. The specific heat of water is 4.184 J K -1 g -1 and the heat capacity...

(a) We place 119.5 g of a metal at 25.00^oC in 423.8 g of water at 95.00^oC. The water is in a beaker that is also at 95.00^oC. The specific heat of water is 4.184 J K^-1 g^-1 and the heat capacity of the beaker is 0.4444 kJ K^-1. The specific heat capacity of the metal is 0.5555 J K^-1 g^-1. What is the final temperature of the metal, the water, and the beaker?


(b)For the oxidation of exactly one mole of a metal, M(s),


          M(s) + (3/2) O₂(g) → MO₃(s)


under a constant pressure of 1.00 atm and a temperature of 25.0^oC, the value of ΔH is -49.2 kJ. What are the values of ΔU, Q, and W for this oxidation under these conditions?