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A 10.0 gram sample of silver is heated to 100.0 degree C and then added to 20.0 g of water at 23.0 C, in an insulated container. At thermal equilibrium, the temperature of the system was measured and found to be 25.0 C. What is the specific heat, Cs, of silver?

Respuesta :

Answer:

[tex]C_{Silver}=0.2231\ J/g^0C[/tex]

Explanation:

Considering that:-

Heat gain by water = Heat lost by Silver

Thus,  

[tex]m_{water}\times C_{water}\times (T_f-T_i)=-m_{Silver}\times C_{Silver}\times (T_f-T_i)[/tex]

Where, negative sign signifies heat loss

Or,  

[tex]m_{water}\times C_{water}\times (T_f-T_i)=m_{Silver}\times C_{Silver}\times (T_i-T_f)[/tex]

For water:

Mass = 20.0 g

Initial temperature = 23.0 °C

Final temperature = 25.0 °C

Specific heat of water = 4.184 J/g°C

For Silver:

Mass = 10.0 g

Initial temperature = 100.0 °C

Final temperature = 25.0 °C

Specific heat of silver = ?

So,  

[tex]20.0\times 4.184\times (25.0-23.0)=10.0\times C_{Silver}\times (100.0-25.0)[/tex]

[tex]10C_{Silver}\left(100-25\right)=20\times \:2\times \:4.184[/tex]

[tex]10C_{Silver}\left(100-25\right)=167.36[/tex]

[tex]C_{Silver}=0.2231\ J/g^0C[/tex]

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