For the galvanic cell that uses the reaction
2 Al(s) + 3 Ni2+(aq) → 2 Al3+(aq) + 3 Ni(s)
the value of n in the relationship ΔG° = -nFE° is ________.
Isn't it 6.
2Al ==> Al^+ + 6e
so the n value would be 6 moles of e-.
the F is the constant.
E* calculated was 1.41 V.
But i am really unsure if im correct or not.
To find the value of n in the relationship ΔG° = -nFE°, where n represents the number of moles of electrons transferred in the chemical reaction, we need to examine the balanced chemical equation:
2 Al(s) + 3 Ni2+(aq) → 2 Al3+(aq) + 3 Ni(s)
From this equation, we can determine that 3 moles of electrons are transferred for every 2 moles of Al(s) and 3 moles of Ni2+(aq) involved in the reaction.
Therefore, the value of n in the relationship ΔG° = -nFE° is 3.
To determine the value of n in the relationship ΔG° = -nFE° for the given galvanic cell reaction, we need to analyze the balanced chemical equation for the reaction.
The balanced equation for the galvanic cell reaction is:
2 Al(s) + 3 Ni2+(aq) → 2 Al3+(aq) + 3 Ni(s)
In this equation, we can see that for every 2 moles of aluminum (Al) that react, it leads to the formation of 2 moles of aluminum ions (Al3+). Similarly, for every 3 moles of nickel ions (Ni2+) that react, it leads to the formation of 3 moles of nickel (Ni).
To calculate the value of n, we look at the coefficients in the balanced equation. The coefficients represent the number of moles of each species involved in the reaction. In this case, we can see that for every 2 moles of aluminum that react, it produces 6 moles of electrons (from 3 moles of Ni2+ reduced to 3 moles of Ni). Therefore, the value of n is 6.
Hence, in the relationship ΔG° = -nFE°, the value of n for the given galvanic cell reaction is 6.