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1st reaction: solid iodine + gaseous chlorine → solid iodine monochloride
Balanced reaction: I2(s) + Cl2(g) → 2 ICl(s)
2nd reaction: treatment of the solid with more chlorine gas
Balanced reaction: 2 ICl(s) + 2 Cl2(g) → 2 ICl3(s)
1 mol of iodine produces 2 moles of ICl and 2 moles of ICl produces to moles of ICl3
molar mass ICl3 = 233.25 g/mol
molar mass I2 = 253.8 g/mol
Solid iodine trichloride is prepared in two steps: first, a reaction between solid iodine and gaseous chlorine to form solid iodine monochloride; second, treatment of the solid with more chlorine gas.
(c) How many grams of iodine are needed to prepare 2.45 kg of final product?
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