The following data was obtained for Part B of the lab: Mass of Cu before electro

ID: 1085137 • Letter: T

Question

The following data was obtained for Part B of the lab:

Mass of Cu before electrolysis = 21.1301 g

Mass of Cu after electrolysis = 20.9894 g

Time of electrolysis = 464 sec

Average current = 0.92 Amp

Volume of gas collected = 54.1 mL

Atmospheric pressure (corrected to standard conditions) = 760.3 mmHg

Room temperature = 18.7 °C

Vapour pressure of water at 18.7 °C = 16.1 mmHg

Using this data determine:

Moles of Cu consumed:___moles

Moles of H2 produced:___moles

Experimental value of Faraday’s constant based on Cu consumed:___C/mole e-

Experimental value of Avogadro’s number using the charge of one electron (1.602 x 10-19 C)?

Mass of Cu before electrolysis = 21.1301 g

Mass of Cu after electrolysis = 20.9894 g

so mass of Cu consumed = (21.1301 - 20.9894) = 0.1407 gm.

0.1407 gm Cu = mass / molar mass = 0.1407 / 63.5 = 0.0022 mole. = 2.2 * 10^-3 mole coppers consumed.

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