In an electrolysis cell similar to the one employed in this experiment, a studen

Question

In an electrolysis cell similar to the one employed in this experiment, a student observed that his unknown metal anode lost 0.208 g while a total volume of 96.30 ml. of H_2 was being produced The temperature in the laboratory was 25 degree C and the barometric pressure was 748 mm Hg. At 25 degree C the vapor pressure of water is 23.8 mm Hg. To find the equivalent mass of his metal, he filled in the blanks below. Fill in the blanks as he did. P_H_2 = P_bar - VP_H_2O = mm Hg = atm V_H_2 = mL = L T = K n_H_2 = moles n_H_2 = PV/RT (where P = P_H_2) 1 mole H_2 requires passage of faradays No. of faradays passed = Loss of mass of metal anode = g No. grams of metal lost per faraday passed = no. grams lost/no. faradays passed = g = EM The student was told that his metal anode was made of iron. MM Fe = g. The charge n on the Fe ion is therefore. (See Eq. 31.) In ordinary units, the faraday is equal to 96,480 coulombs. A coulomb is the amount of electricity passed when a current of one ampere flows for one second. Given the charge on an electron, 1.6022 Times 10^-19 coulombs. calculate a value for Avogadro's number.

Explanation / Answer

2.

You need to divide Faraday's constant by Charge of an electron
Faraday's constant = 96,485.3383=9.64853383 * 10^4 in scientific notation
Charge of an electron = 1.60217646 × 10(-19) which is already in scientific notation
now
divide 9.64853383 by 1.60217646 to get
6.0221417995368625001518247247248 which you cut off at 8 decimal points to 6.02214179
now divide 10^4 by 10^(-19) to get 10^(4-(-19))=10^23
Thus your answer is 6.02214179*10^23 for an accurate value of Avogadro's number.

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