c. If a piece of jewelry were electroplated with gold for 25 seconds at 1.5 A, how many grams of gold would be plated? (Note: 1 A = 6.241 1018 e–/s. The reaction for the reduction of gold ions to gold metal is Au+ + 1e– Au(s).) (1 point)
Reaction is Au+ + 1e– -> Au(s) Figure out how many electrons are put into the reaction in 25 seconds at 1.5 A, this will equal the amount of Au(s) atoms you produce from atoms using avagadros number you can find moles from moles you can find grams
Any questions?
If you are having trouble with the math let me know I can help you through it
here's what i have so far.. 1 A = 6.241 1018 e–/s so…. 1.5(6.241 x 1018 e-/s)25s = number of atoms reduced number of atoms reduced = 2.34 E 20
so do i multiply that by avogrado's number(6.0221413e+23)
so 2.34 E 20*6.0221413e+23)
1.4091811e+24 moles right?
no wait i did this wrong
http://www.wolframalpha.com/input/?i=1.5%286.241+x+10^18+e-%2Fs%2925 Yeah you messed up the first calculation
i did plug that into my calculator but i must've misread something
number of atoms reduced 6.362*10^20
yep i got that
and then multiply by avogadro's #?
dont i need to find the mass of gold?
Yes but if you multiply you are going to get an absurd number, Avogadro's number has units, 6.022141*10^23 atom/mol
you will end up with atom^2/mol which is not useful
as units
1.4091811e+24 moles is 3.8*mass of the moon lol that is a lot of gold
oh wow yea haha
always pay attention to number sizes in chemistry and really any science
i realized i multiplied by 1018 instead of 10^18 it was a typo
Au+ + 1e– has to be used next...?
not really a big deal you can tell the number was in scientific notation
well it is a 1 to 1 reaction thus the number of electrons reacted = number of Au(s) produced
so you can just say that the number of electrons = number of atoms of Au(s) produced
i think my teacher said we have to convert this to moles and then grams.
yes you convert to moles using avagadros number
i know that for grams it's : mol of substance x (Atomic mass of substance/ 1 mol)
oh so i have to use avogadros #
so from above, we know that there are 6.362x10^20 atoms reduced. so i multiply this by avogadro's number right?
well look at the units of your two numbers avagadros number: 6.022141*10^23 atom/mol number of Au(s) atoms: 6.362*10^20 atom you need to set these numbers up so you end up with just the units mole, remember just like numbers units can cancel out when divded and can be raised to powers when multiplied together
oh okay i got it!
so its 1.056434912x10^-3
moles*
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