Question

2. In Part A of the experiment, what amount of "unknown metal" should be used? How is the precise mass of the "unknown metal determined? 3. In Part A of the experiment, why must the "unknown metal" initially be completely dry? How is it kept dry during heating? Determine the specific heat of an unknown metal following a procedure similar to Part A, using the data given: A 35.3g sample of metal was heated in a water bath to 99.5°C. When the hot metal was added to a sample of water (23.2g), the temperature of the water increased from 21.3°C to a max temperature of 27.5°C (obtained from graph). a. Mass of metal: b. Mass of water: c. Initial temperature of water in calorimeter (Z of water): d. Initial temperature of metal (boiling water) (of metal): c. Maximum temperature of metal and water mixture (°C): f. AT of water (°C): Show calculation: B. AT of metal (°C): Show calculation: h. Heat gained by water (J) using equation 2: Show calculation:

Answer 1

4) In calorimeter, heat lost by metal is equal to heat gained by water.

Given, mass of metal(Mm) = 35.3 g

DT of metal = 99.5 - 27.5 = 72 oC

mass of water(Mw) = 23.2 g

DT of water = 27.5 - 21.3 = 6.2 oC

Specific heat of water(Cw) = 4.186 J/ g oC

Heat gained by water = Mw * Cw * DT

= 23.2*4.186*6.2

= 602.1 J

Heat lost by metal = heat gained by water

Mm * Cm * DT = 602.1

35.3*Cm*72 = 602.1

Cm = 0.237 J/g oC

So, specific heat of the metal is 0.237 J/g oC.

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