Question

An irregular lump of an unknown metal has a measured density of 3.84 g/mL. The metal is heated to a temperature of 161 °C and placed in a graduated cylinder filled with 25.0 mL of water at 25.0 °C. After the system has reached thermal equilibrium, the volume in the cylinder is read at 33.7 mL, and the temperature is recorded as 37.4 °C. What is the specific heat of the unknown metal sample? Assume no heat is lost to the surroundings. A solution is made by mixing 209.0 mL of ethanol initially at 11.3 ∘ C with 209.0 mL of water initially at 24.9 ∘ C . What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL . The specific heat of ethanol is 2.46 J / g⋅°C and the specific heat of water is 4.184 J / g⋅°C .

Answer 1

volume of unknown metal = (33.7 -25.0) = 8 8.7 ml mans of unknown metal = density xvolume = 3.84 x 8.7 = 33.408g heat release by metal = heat absorb by water 33.408 X Cm X (161-374) = 25 X 4,184 x (37,4-25) - = specific head of metal = cm = 0.314 5/9°C - mass of ethanda 209.0x0,789 = 169.901 g man o waters 209.0x1.00 - 200 g heat absorb by ethanol = heat release be water = 164.901 X 2.46*(T-11.3) = 20984.184X (29-9-T) =) T = 20.59°C (final temperahse)

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