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Tasya [4]
3 years ago
14

An irregular lump of an unknown metal has a measured density of 5.50 g/mL. The metal is heated to a temperature of 153 °C and pl

aced 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 30.0 mL, and the temperature is recorded as 41.0 °C. What is the specific heat of the unknown metal sample? Assume no heat is lost to the surroundings.
Chemistry
1 answer:
Oliga [24]3 years ago
7 0

Answer: 0.543J/g^0C

Explanation:

Volume of metal = volume of water displaced = (30.0 - 25.0) ml = 5.0 ml

Density of metal = 5.50 g/ml

Mass of metal =density\times volume =5.50\times 5.0=27.5g

Volume of water = 25.0 ml

Density of metal = 1.0 g/ml

Mass of metal =density\times volume =1.0\times 25.0=25.0g

heat_{absorbed}=heat_{released}

As we know that,  

Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})

-[m_1\times c_1\times (T_{final}-T_1)]=[m_2\times c_2\times (T_{final}-T_2)]         .................(1)

where,

q = heat absorbed or released

m_1 = mass of metal = 27.5 g

m_2 = mass of water = 25.0 g

T_{final} = final temperature = ?41.0^0C

T_1 = temperature of metal = 153^oC

T_2 = temperature of water = 25.0^oC

c_1 = specific heat of lead = ?

c_2 = specific heat of water= 4.184J/g^0C

Now put all the given values in equation (1), we get

27.5g\times c_1\times (41.0-153)^0C=[25.0g\times 4.814J/g^0C\times (41.0-25.0)^0C]

c_1=0.543J/g^0C

Thus the specific heat of the unknown metal sample is 0.543J/g^0C

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