Q= I * t where I = current , t = time , Q = amount of electric charge.
K2Cr2O7 --------------> Cr which is Cr6+ + 6electrons --------------> Cr (metal)
So, to produce 1 mole of Cr metal, 6 moles of electronic charge is required, which is 6 * 96500 C.
Now, we shall calculate number of moles of Cr:
Number of moles = mass / molar mass = 2.91 * 10 -3 g / 51.996
= 0.05596 * 10 -3 moles.
to produce 1 mole of Cr metal, 6 * 96500 C moles of electronic charge is required
therfore for 0.05596 * 10 -3 moles of Cr metal, charge required = 6 * 96500 * 0.05596 * 10 -3
= 32.40084 C of electronic charge.
Q= I * t
time = Q / I = 32.40084 C / 0.580 A = 55.8635 seconds
Question 6 (1 point) How many seconds are required to produce 2.91 mg of chromium metal...
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