Electrolysis can be used to determine atomic masses. A current of \(0.550\) A deposits \(0.55 \mathrm{~g}\) of a certain metal in 100 minutes. Calculate the atomic mass of the metal if eq. wt. = mole. wt./3 (a) 100 (b) \(45.0\) (c) \(48.25\) (d) \(144.75\)

Understanding chemical calculations is an integral part of mastering chemistry, especially when delving into concepts such as electrolysis. These calculations are necessary for predicting the outcome of reactions and understanding the quantitative aspects of chemical processes. When we discuss the context of electrolysis, we must become familiar with Faraday's laws of electrolysis, which provide the quantitative basis to relate the amount of substance deposited on an electrode to the quantity of electric charge passed through the solution.

Let's consider the problem presented. It involves calculating the atomic mass of a metal based on the amount of metal deposited during electrolysis. To approach this problem systematically, we apply chemical calculations using the formula derived from Faraday's law:
\( m = \frac{MIt}{nF} \)
Where each variable represents a specific quantity: mass deposited (m), molar mass (M), electric current (I), time (t), valence number (n), and Faraday's constant (F). By rearranging the equation and plugging in known values, we can solve for the unknown molar mass of the metal.

Performing these calculations correctly is essential for students to understand not only the specific procedure in question but also the broader application of fundamental chemical principles in practical scenarios like electrochemical deposition.

Molar mass determination is a key concept in chemistry that allows us to understand the relationship between the mass of a substance and the amount of substance present in moles. In an electrolysis experiment, accurately determining the molar mass is crucial because it helps identify the substance being deposited. This process also showcases the importance of stoichiometry and chemical calculations in everyday laboratory practices.

According to the problem we have, the equivalent weight of a substance is indicated to be one-third of the molecular weight (eq. wt. = mole wt./3). This piece of information, combined with Faraday's law, gives us insight into how to calculate the molar mass of the metal. Equivalent weight relates to the molar mass divided by the valence; thus, we can infer that the valence for our substance is three. By utilizing the electrolysis formula and solving for the molar mass (M), students can determine the molar mass of the unknown metal to be approximately 48.25 g/mol.

Understanding how to calculate molar mass directly from experimental data, as in the case of electrochemical deposition, not only reinforces the student's understanding of theoretical concepts but also provides valuable laboratory skills.

Electrochemical deposition is a fascinating process where material from an electrolyte is deposited onto an electrode due to the flow of electric current. This process is not only vital for determining chemical properties like atomic mass but also has widespread applications in industries for plating, corrosion protection, and manufacturing of electronic components.

In the context of our problem, electrochemical deposition is used to deposit a known mass of a metal from its ionic solution. By measuring the mass of the deposited metal and knowing the amount of electric current used, we can apply Faraday's law to determine properties such as the metal's atomic or molar mass. This experimentally-driven method allows for the direct verification of theoretical molecular weights, highlighting the synergistic relationship between theoretical concepts and practical applications. Through such hands-on experiments, students can witness firsthand the principles of chemistry in action, cementing their understanding of both the scientific theory and the methodology behind determining chemical properties via electrochemical means.