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oksian1 [2.3K]
3 years ago
9

A standard galvanic cell is constructed so that the overall cell reaction is as given below where M is an unknown metal. 2 Al3+(

aq) + 3 M(s) 3 M2+(aq) + 2 Al(s) If ΔG° = -411 kJ for the overall cell reaction, identify the metal used to construct the standard cell.
Chemistry
1 answer:
jasenka [17]3 years ago
5 0

Answer:

magnesium metal

Explanation:

According to the redox reaction equation, six electrons were transferred hence n=6 and F= Faraday's constant 96500C. ∆G° is given hence E°cell can easily be calculated as follows:

From ∆G°= -nFE°cell

E°cell= -∆G°/nF= -(-411×10^3/96500×6)

E°cell= 0.7098V

But for Al3+(aq)/Al(s) half cell, E°= -1.66V from standard table of reduction potentials.

E°cell= E°cathode- E°anode but Al3+(aq)/Al(s) half cell is the cathode

Hence

E°anode=E°cathode - E°cell

E°anode= -1.66-0.7098= -2.37V

This is the reduction potential of Mg hence the anode material was magnesium metal

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Step 2:

Conversion of 75.0 mL of H2O to Litre (L).

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Therefore, 75mL = 75/1000 = 0.075L

Step 3:

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Molarity is simply defined as the mole of solute per unit litre of water. Mathematically, it is represented as:

Molarity = mole /Volume

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