Could you please help me to do the calculation for trail one . I. Measurements C

Question

Could you please help me to do the calculation for trail one . I. Measurements Current 1min. 2min. 3min. 4min. 5min. 6min. 7min. 8min. Trial 3 Trial 1 Trial 2 Trial 3 Total time of electrolysis. Volume of H2. Barometric pressure. Temperature of the solution. Height of the solution column. Il. Calculations: min 787.64 787 Su 23-2 23-9 220 173 Trial 2 Trial 3 Trial 1* Average current. Charge passed. Vapor pressure of water (see Table below). Partial pressure of H2 Moles of H2(g) produced. Moles of electrons Faraday Constant(experimental value). Number of electrons passed. Avogadro's Number (experimental value) Show calculations for Trial 1 on a separate sheet of paper.

Explanation / Answer

For trial 1:

Average current = 0.156 A

Charge passed = Avg current*Time = 0.156*(8*60) = 74.88 C

At the given temp, Vapor pressure of water = 21.3 torr = 21.3 mm Hg

Partial pressure of hydrogen = 787.654-21.3 = 766.354 mm Hg

Putting values in the ideal gas equation:

PV = nRT

(766.354/760)*0.0097 = n*0.0821*300.2

Solving we get:

n = 0.000397

Since 1 mole of hydrogen gas is produced using two moles of electrons, so moles of electrons passed = 0.000397*2 = 0.000794

Experimental value of Faraday's constant = Charge passed/Moles of e- = 74.88/0.000794 = 94307.30 C/mol e-

Hope this helps !

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