<p>How many faradays of electricity are involved in each of the following electrochemical reactions?</p>
<p>(a) 0.500 mol of Br2 are converted to Br-
(b) 2.0 L of O2 at STP are converted to H2O in acid solution</p>
<p>I'm really stuck :(</p>
<p>1 faraday = 96500 coulombs per mole of electrons</p>
<p>so,</p>
<p>(a) Br2 –> 2Br-</p>
<p>since the mole ratio is 1:2, 2(.500 mol Br2)=1 mole of Br-, and since it is only reduced by one, 1 farraday is involved in this reaction</p>
<p>(b) 2O2 + 4H+ –> 2 H2O</p>
<p>okay, so 2L of O2 = 2L/22.4L/mol = .0893 mol O2. Since the mole ratio is constant, you don;t have to multiply because of that. However, O2 is reduced to a -2 oxidation number so 2(.0893 mol)=0.179 mol of electrons= 0.179 Farradays. </p>
<p>Hope this helps!</p>
<p>isnt the answer for b 0.356 farradays? because isnt the equation 2H20=4H^(+) + O2 + 4e-?</p>
<p>ohhh crap yeah… You’d think by the end of AP Chem I could balance an equation :-P</p>