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expeople1 [14]
2 years ago
11

Calculate the heat required to form a liquid solution at 1356 k starting with 1 mole of cu and 1 mole of ag at 298 k. at 1356 k

the molar heat of mixing of liquid cu and liquid ag is given δhm = 20,590xcuxag .
Chemistry
1 answer:
tatyana61 [14]2 years ago
3 0

Answer:

Q=87924J

Explanation:

Hello,

At first, we must consider that at the beginning, both copper and silver are solid, so we must melt both of them, thus, the following enthalpic routes are proposed in order to know each heat because coppers melting points as a value of 1356K and silver's melting point 1235K:

H_{Cu}=n_{Cu}*(Cp_{solid,Cu}(T_2-T_1)+H_{melt})\\H_{Cu}=1mol*(0.3768J/gK*63.546g/mol*(1356-298)K+13590J/mol) \\H_{Cu}=38922.89J

H_{Ag}=n_{Ag}*(Cp_{solid,Ag}(T_m-T_1)+H_{melt}+Cp_{liquid,Ag}(T_2-T_m))\\H_{Ag}=1mol*(0.235J/gK*107.868g/mol*(1235-298)K+11300J/mol+0.28J/gK*107.868g/mol*(1356-1235)K) \\H_{Ag}=38706.56J

Now, the released heat due to the mixing process turns out into:

H_{mix}=2mol*(20590x_{Cu}x_{Ag}J/mol)\\H_{mix}=2mol*20590(0.5)(0.5)J/mol\\H_{mix}=10295J

Finally, the total heat required is found by:

Q=H_{Cu}+H_{Ag}+H_{mix}\\Q=38922.89J+38706.56J+10295J\\Q=87924J

Best regards.

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