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Natasha_Volkova [10]
3 years ago
12

Calculate the cell potential, Ecell, of a concentration cell containing a 0.1 M solution of Zn2 and a 1.0 M solution of Zn2

Chemistry
1 answer:
Agata [3.3K]3 years ago
3 0

Answer:

The cell potential is 0.0296V

Explanation:

Please see the attachment below

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Read 2 more answers
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
tatyana61 [14]

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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4 years ago
How fast a reactant is used up to how fast a product is formed is _____.
STatiana [176]

Answer:   B) The rate of reaction

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The equilibrium explains that how much concentration of reactant is in equilibrium with the product.

Solution concentration is the number of moles of solution divided by volume.

The catalyst is the substance which increases the rate of the reaction which bringing any change in other things.

5 0
3 years ago
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