Question

A 102.5 g sample of metal beads was heated in a water bath to 99.5deg. Celsius. The metal was then added to a sample of water (25.7g) and the temperature of the water changed from an initial temperature of 20.0 deg. Celsius to a final temperature of 41.5 degree Celsius.

A) What was the temperature of the metal at equilibrium?

B) What was the temperature change of the metal?

C) Calculate the specific heat and the atomic mass of the metal. What is the metal?

Answer #1

A)

mass of metal = 102. 5 g

initial temperature of metal = 99.5 oC

initial temperature of water = 20

final temperature of water = 41.5 oC

**temperature of the metal at equilibrium = 41.5
oC**

B)

temperature change of metal = 99.5 - 41.5

**temperature change of metal = 58 oC**

C)

here

heat loss by metal = heat gain by water

m Cp dT = m Cp dT

102.5 x Cp x 58 = 25.7 x 4.184 x (41.5 - 20)

Cp = 0.389 J/ goC

**specific heat of metal = 0.389 J / g oC**

**the metal is Zinc (Zn)**

**atomic mass of metal = 65.38 g/mol**

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