Cu + 2H+ (aq) ===> Cu2+ (aq) + H2 (g)
#1 . moles of H2 produced , form PV = nRT
n = PV/RT
P = 710.9 / 760 mmHg/atm = 0.9354 atm
n = 0.9354 atm *0.03502 L / 0.0821 L-atm/K-mol * 295.15 K = 1.35*10-3 moles
1 mol of H2 = 1 mol of Cu
moles of Cu consumed = 1.35*10-3 moles
similarly , trial #2 : moles of Cu consumed = 1.31*10-3 moles
==
#2.
#1. Number of coulombs = current in amps x time in seconds = 0.135 A * 1837 s = 247.96 C
1 mole of H2 = 2 mol of electrons
moles of Electrons : 2.7*10-3 moles
thus, Faraday = 247.96 C/ 2.7*10-3 moles= 91,837 C/mol
#2 : Faraday = 91,375 C/mol
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#3 #1 atomic mass of Cu : mass of Cu consumed / moles of Cu consumed = 0.088 g/ 1.35*10-3 moles = 65.2 g/mol
#2 . atomic mass of Cu : 63.4 g/mol
==
#4 AVERAGE value Faraday : 91606 C/mol
% error : / 96488 - 91606 / / 96488 *100 = 5.06 %
i need help with these questions. QuesL # Deductions ol OL Total Constant Current System #...
Need help filling in my data sheet from a lab. My professor said
the pressure was 24.6 inches of Hg and that we needed to convert
that to moles. Im not sure i put that in the correct spot. I
included the lab protocol. Plz plz plz help me fill in the blanks
and let me know if i did something wrong Im very confused haha.
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