if 4.4 moles of copper metal was deposited from a solution of Cu(NO3)2, how many electrons were involved?
To determine the number of electrons involved in the deposition of 4.4 moles of copper metal, we can start by understanding the reaction taking place.
The chemical equation for the reaction between copper(II) nitrate (Cu(NO3)2) and the deposition of copper metal (Cu) is as follows:
2Cu(NO3)2(aq) + 2e- → 2Cu(s) + 4NO3-(aq)
From the equation, it is evident that for every two moles of copper nitrate that react, two moles of electrons are involved in the reduction process. This means that the stoichiometric ratio of moles of electrons to moles of copper metal is 2:2, or 1:1.
Since we know that 4.4 moles of copper metal were deposited, we can conclude that the same number of electrons were involved. Therefore, 4.4 moles of electrons were required for the deposition of 4.4 moles of copper metal.
To determine the number of electrons involved in the deposition of 4.4 moles of copper, we need to use the balanced equation for the electrodeposition of copper:
Cu^2+ + 2e^- -> Cu
From the equation, we can see that for every 2 moles of electrons, 1 mole of copper is deposited.
Therefore, we can set up a ratio between moles of electrons and moles of copper:
2 moles electrons / 1 mole copper
Using this ratio, we can determine the number of moles of electrons involved:
Number of moles of electrons = 4.4 moles copper x (2 moles electrons / 1 mole copper)
Number of moles of electrons = 8.8 moles electrons
So, 8.8 moles of electrons are involved in the deposition of 4.4 moles of copper.