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Anuta_ua [19.1K]
1 year ago
14

A concentration cell is constructed using two NI electrodes with Ni2 concentration of 1. 0 m and 1. 0 x 10^-4 m in the two half-

cells. Calculate the potential of the cell if the reaction is spontaneous
Chemistry
1 answer:
Crank1 year ago
6 0

The potential of the concentration cell is 0.1182 V when the reaction is spontaneous.

<h3>What is Concentration Cell?</h3>

An electrolytic cell that contains two half cells with the same electrodes but with different concentrations is known as a concentration cell.

<h3>What is Nernst Equation?</h3>

Nernst Equation helps in determining the cell potential under the non-standard conditions that are at any known temperature, pressure, and concentration. It is given by

E = E^o - \frac{2.303RT}{F} log Q

At T = 298 K,

E = E^o - \frac{0.0591}{n} logQ

For Ni concentration cell, anode and cathode are the same and thus E° is zero

At anode,

Ni (s)\rightarrow Ni^2^+ + 2e^-

At Cathode,

Ni^2^+ + 2e^-\rightarrow Ni (s)

No of moles of electrons, n = 2

Then, the potential of the cell is given by

E=- \frac{0.0591}{n} logQ

Q = \frac{[diluted Ni]}{[concentrated Ni]}

diluted Ni = 1 x 10⁻⁴ M and concentrated Ni = 1 M

E = \frac{-0.059}{2} log\frac{ 10^-^4}{1}\\   = \frac{-0.059}{2} \times -4 log10

log(10) = 1

E = 0.1182 V

Hence, the potential of the cell is 0.1182 V.

Learn more about the Nernst equation:

brainly.com/question/15237843

#SPJ4

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Glycerol (C3H8O3), also called glycerine, is widely used in the food and pharmaceutical industries. Glycerol is polar and dissol
Stells [14]

Here is the complete question.

Glycerol (C3H8O3), also called glycerine, is widely used in the food and pharmaceutical industries. Glycerol is polar and dissolves readily in water and polar organic solvents like ethanol. Calculate the mole fraction of the solvent in a solution that contains 1.61 g glycerol dissolved in 22.60 mL ethanol (CH3CH2OH; density = 0.7893 g/mol). Round to four significant digits

Answer:

0.9567 mol

Explanation:

Given that:

mass of glycerol = 1.61 g

molar mass of glycerol = 92.1 g/mol

no of mole = \frac{mass}{molar mass}

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= 0.0175 mol

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Density of ethanol = 0.7893 g/mL

Since Density = \frac{mass}{volume}

∴  mass of ethanol = density of ethanol × volume of ethanol

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mass of ethanol =  17.838 g

Number of moles of ethanol (n_{ethanol}) = \frac{17.838}{46.0684}

= 0.387 mole

∴ the mole fraction of the solvent can be determined as:

X_{solvent} = X_{ethanol} = \frac{n_{ethanol}}{n_{glycerol}+n_{ethanol}}

=\frac{0.387 mol}{(0.0175+0.387)mol}

= \frac{0.387mol}{0.4045mol}

= 0.95673671199

≅ 0.9567 mol

∴ The mole fraction of the solvent in a solution that contains 1.61 g glycerol dissolved in 22.60 mL ethanol is = 0.9567 mol

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