An unknown metal (M)is electrolyzed.It took 74.1 s for a current of 2.00 amp to plate 0.107 g of the metal from a solution containing M(NO₃)₃.Identify the metal.

Question

Quizplus · Accepted Answer

First, we need to calculate the amount of charge that passed through the electrolytic cell using Faraday's Law:

Q = It
Q = (2 A) x (74.1 s)
Q = 148.2 C

Next, we can use the charge and the mass of the metal deposited to calculate the molar mass of the metal:

mol M = Q / nF

n = mass / molar mass

mol M = (148.2 C) / (1 mol e⁻/ 96485 C) x (0.107 g / M)

Solving for molar mass, we get:

M = 208.2 g/mol

Based on the answer choices, the closest match to this molar mass is Bi (which has a molar mass of 208.98 g/mol). Therefore, the unknown metal M is likely bismuth (Bi).

An Unknown Metal (M)is Electrolyzed