A battery is constructed based on the oxidation of magnesium and the reduction of Cu2+. The initial concentrations of Mg2+ and Cu2+ are 1.0×10−4 M and 1.6 M , respectively, in 1.0-liter half-cells.

What is the initial voltage of the battery?

The initial voltage of the battery is 2.83 V

From the reduction potential table, the standard reduction potential values, E° of Mg²⁺ and Cu²⁺ are -2.37 and +0.34 respectively.

Since magnesium is oxidized and copper is reduced, the equation of the reaction is given as:

Mg (s) + Cu²⁺ (aq) > Mg²⁺ (aq) + Cu (s)

E° of cell is given as: E°(oxidized) + E°(reduced)

E° of cell = 2.37 +0.34 = 2.71 V

The initial concentrations of Mg²⁺ and Cu²⁺ are 1.0 × 10⁻⁴ M and 1.6 M

Using the Nernst Equation:

Ecell = E° - 0.0592/n * logQ

n = 2 moles of electrons

Q = [Mg²⁺]/[Cu²⁺]

Q = 1.0 × 10⁻⁴ M / 1.6 M = 6.25 * 10⁻⁵

Ecell = 2.71 - (0.0592/2) * log 6.25 * 10⁻⁵

Ecell = 2.83 V

Therefore, the initial voltage of the battery is 2.83 V

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2.59 V

Explanation:

Equation of the reaction:

Mg(s) + Cu^2+(aq) > Mg^2+(aq) + Cu(s)

From Nernst Equation

E= E°-0.0592/n log [Red]/ [Ox]

E°= 0.34- (-2.37)= 2.71

E= 2.71 - 0.0592/2 log [1.6]/ [1×10^-4]

E= 2.71 - 0.12

E= 2.59 V

h let me think

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.