This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Here's the solution using a method commonly found in chemistry textbooks, breaking down the steps to calculate the oxidation state. Given: Current (I) = 3.0 A Time (t) = 4 hours Mass of tin deposited (m_Sn) = 26.6 g Molar mass of tin (M_Sn) = 119 g/mol Faraday's constant (F) = 96500 C/mol Goal: Determine the oxidation state of tin, which is the number of electrons (z) involved in the reduction of tin ions to tin metal. The general half-reaction is Sn^z+ + ze^- Sn(s). Step 1: Convert time from hours to seconds. t = 4 hours × 60 minutes1 hour × 60 seconds1 minute t = 14400 s Step 2: Calculate the total quantity of electricity (charge, Q) passed. The formula for charge is Q = I × t. Q = 3.0 A × 14400 s Q = 43200 C Step 3: Calculate the moles of tin (Sn) deposited. The formula for moles is n = massmolar mass. n_Sn = 26.6 g119 g/mol n_Sn ≈ 0.223529 mol Step 4: Calculate the moles of electrons (n_e) transferred. One mole of electrons carries a charge equal to Faraday's constant (F). n_e = (Q)/(F) n_e = 43200 C96500 C/mol n_e ≈ 0.447668 mol Step 5: Determine the oxidation state (z) of tin. From the half-reaction Sn^z+ + ze^- Sn(s), we know that z moles of electrons are required to deposit 1 mole of tin. Therefore, the ratio of moles of electrons to moles of tin gives the oxidation state. z = (n_e)/(n_Sn) z = 0.447668 mol0.223529 mol z ≈ 2.0027 Rounding to the nearest whole number, as oxidation states are typically integers: z = 2 The oxidation state of tin in the salt is +2.