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Simora [160]
3 years ago
5

You placed 43.1 g of an unknown metal at 100 °C into a coffee cup calorimeter that contained 50.0 g of water that was initially

at 22.0 °C. The equilibrium temperature of mixing (T0) was determined to be 23.2 °C. The calorimeter constant was known to be 51.5 J/°C. Specific HeatH2O = 4.184 J/g·°Ca. What is the total amount of heat (J) lost by the metal? NG 1.5b. What was the specific heat (J/g·°C) of the metal? NG 1.5
Chemistry
1 answer:
nika2105 [10]3 years ago
8 0

Answer :

(a) The heat released by the metal is -312.48 J

(b) The specific heat of the metal is 0.0944J/g^oC

Explanation :

<u>For part A :</u>

Heat released by the metal = Heat absorbed by the calorimeter + Heat absorbed by the water

q=[q_1+q_2]

q=[c_1\times \Delta T+m_2\times c_2\times \Delta T]

where,

q = heat released by the metal

q_1 = heat absorbed by the calorimeter

q_2 = heat absorbed by the water

c_1 = specific heat of calorimeter = 51.5J/^oC

c_2 = specific heat of water = 4.184J/g^oC

m_2 = mass of water = 50.0 g

\Delta T = change in temperature = (T_{final}-T_{initial})=23.2-22.0=1.2^oC

Now put all the given values in the above formula, we get:

q=[(51.5J/^oC\times 1.2^oC)+(50.0g\times 4.184J/g^oC\times 1.2^oC)]

q=312.48J

Thus, the heat released by the metal is -312.48 J

<u>For part B :</u>

q=m\times c\times \Delta T

q = heat released by the metal = -312.48 J

m = mass of metal = 43.1 g

c = specific heat of metal = ?

\Delta T = change in temperature = (T_{final}-T_{initial})=23.2-100=76.8^oC

Now put all the given values in the above formula, we get:

-312.48J=43.1g\times c\times 76.8^oC

c=0.0944J/g^oC

Thus, the specific heat of the metal is 0.0944J/g^oC

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