Propagation of uncertainty. In an extremely accurate measurement of the Faraday constant, a pure silver anode was oxidized to Ag1 with a constant current of 0.203 639 0 (60.000 000 4) A for 18 000.075 (60.010) s to give a mass loss of 4.097 900 (60.000 003) g from the anode. Given that the atomic mass of Ag is 107.868 2 (60.000 2), find the value of the Faraday constant and its uncertainty.
Propagation of uncertainty. In an extremely accurate measurement of the Faraday constant, a pure silver anode was oxidized to Ag1 with a constant current of 0.203 639 0 (60.000 000 4) A for 18 000.075 (60.010) s to give a mass loss of 4.097 900 (60.000 003) g from the anode. Given that the atomic mass of Ag is 107.868 2 (60.000 2), find the value of the Faraday constant and its uncertainty.
Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry
Section: Chapter Questions
Problem 22.25QAP
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Propagation of uncertainty. In an extremely accurate measurement of the Faraday constant, a pure silver anode was oxidized to Ag1 with a constant current of 0.203 639 0 (60.000 000 4) A for 18 000.075 (60.010) s to give a mass loss of 4.097 900 (60.000 003) g from the anode. Given that the
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