A constant current of 1.50 amp is passed through an electrolytic cell containing a 0.10 M soluti

step 1 A constant current of 1 .50 ampere passed through an electrolytic cell which contains 0 .10 mola

A constant current of 1.50 amp is passed through an...

A constant current of $1.50 \mathrm{amp}$ is passed through an electrolytic cell containing a $0.10 M$ solution of $\mathrm{AgNO}_{3}$ and a silver anode and a platinum cathode until $2.48 \mathrm{~g}$ of silver is deposited. a. How long does the current flow to obtain this deposit? b. What mass of chromium would be deposited in a similar cell containing $0.10 M \mathrm{Cr}^{3+}$ if the same amount of current were used?

A constant current of $1.50 \mathrm{amp}$ is passed through an electrolytic cell containing a $0.10 M$ solution of $\mathrm{AgNO}_{3}$ and a silver anode and a platinum cathode until $2.48 \mathrm{~g}$ of silver is deposited.
a. How long does the current flow to obtain this deposit?
b. What mass of chromium would be deposited in a similar cell containing $0.10 M \mathrm{Cr}^{3+}$ if the same amount of current were used?

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Key Concepts

Electric Current and Charge Relationship

Electric current, measured in amperes, is the rate at which charge flows through a circuit. The total charge (in coulombs) passed is calculated by integrating the current over time, making it fundamental in determining how long an electrolysis process must run to deposit a specific amount of material, as per the relation Q = I × t.

Electrochemical Stoichiometry

This concept involves the quantitative relationship between reactants and products in an electrochemical reaction. It requires understanding the mole ratios of electrons to ions in the redox reaction. For instance, depositing a metal from its ion depends on the number of electrons required to reduce the ion, which is critical when comparing different metals in similar electrolysis setups.

Faraday's Laws of Electrolysis

These laws establish that the amount of substance altered at an electrode during electrolysis is directly proportional to the total electric charge passed through the electrolyte. This principle enables the calculation of the mass of a substance deposited (or dissolved) based on the charge, which is the product of current and time. It also introduces the concept of the equivalence factor, which depends on the number of electrons involved in the redox process.

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