A metal sample weighing 45.2 g and at a temperature of 100.0 °C was placed in 38.6 g of water in a calorimeter at 25.2 °C. At equilibrium the temperature of the water and metal was 33.0 °C.  A) What was ∆t for the water? (∆t= t_final- t_initial)  B) What was ∆t for the metal? C) Taking the specific heat of water to be 4.18 J/g °C, calculate the specific heat of the metal. D) What is the approximate atomic mass of the metal using the equation: MM = 25/S.H.(J/g°C)

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A: Given:65.0 mL of 0.350 M Ba(OH)265.0 mL of 0.700 M HCl.Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O

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