A current of 9.65 amp. passing for 16 min. 40 sec. through a molten tin salt deposits 5.95 gm ofTin. The oxidation state of the tin in the salt is :

To determine the oxidation state of tin in the salt, we can use the concept of Faraday's law of electrolysis.

Step 1: Calculate the total charge passed through the molten tin salt. Given that the current is 9.65 amp and the time is 16 min 40 sec, we need to convert the time to seconds. 16 min 40 sec = (16 x 60) + 40 = 1000 seconds

The total charge passed (Q) can be calculated using the formula: Q = I x t Q = 9.65 amp x 1000 seconds Q = 9650 coulombs

Step 2: Convert the charge passed to the number of moles of electrons. Since 1 Faraday (F) is equal to 96500 coulombs, we can calculate the number of moles of electrons (n) using the formula: n = Q / F n = 9650 coulombs / 96500 coulombs n = 0.1 moles

Step 3: Determine the number of moles of tin deposited. Given that 5.95 grams of tin is deposited, we can calculate the number of moles (m) using the molar mass of tin (Sn), which is 118.71 g/mol. m = mass / molar mass m = 5.95 grams / 118.71 g/mol m = 0.05 moles

Step 4: Determine the oxidation state of tin. The ratio between the number of moles of electrons (n) and the number of moles of tin (m) can give us the oxidation state of tin. If the ratio is 1:1, then the oxidation state is +2. If the ratio is 2:1, then the oxidation state is +4.

In this case, the ratio is 0.1 moles of electrons to 0.05 moles of tin, which simplifies to 2:1. Therefore, the oxidation state of tin in the salt is +4.