This is a confusing one!
How many faradays are required to convert a mole of NO2- ions to NH4+ ions?
a. 4
b. 5
c. 6
d. 7
e. 8
Write the equation and balance
NO2^- ==> NH4^+
electron change actually is all you need and oxidation state goes from +3 in NO2^- to -3 in NH4^+ for 6e change.
Therefore, it will take 1 faraday to convert 1/6 mole NO2^- to NH4^+. So it will take ______ F to convert 1 mole.
To determine how many faradays are required to convert a mole of NO2- ions to NH4+ ions, we need to first understand the stoichiometry of the chemical reaction between NO2- and NH4+. The balanced equation for this reaction should give us the ratio of moles between the reactants and products.
The balanced equation is:
2 NO2-(aq) + 4 H+(aq) + 3 electrons → N2(g) + 2 H2O(l)
From the balanced equation, we can see that for every 2 moles of NO2-, we need 4 moles of H+ and 3 moles of electrons to produce 1 mole of N2.
Since we are interested in converting a mole of NO2- ions to NH4+ ions, we will focus on the reactant side (NO2-) instead of the product side (NH4+). From the balanced equation, we can see that it takes 2 moles of NO2- to produce 1 mole of N2. Therefore, to convert 1 mole of NO2-, we will need to use 2 faradays.
Therefore, the answer is: a. 4 faradays.