Direct reaction of iodine (I2) and chlorine (Cl2) produces an iodine chloride, IxCly, a bright yellow solid. If you completely consume 0.678 g of I2 in a reaction with excess Cl2 and produce 1.246 g of IxCly, what is the empirical formula of the compound? A later experiment showed that the molar mass of IxCly was 467 g.mol-1. What is the molecular formula of the compound?
Direct reaction of iodine (I2) and chlorine (Cl2) produces an iodine chloride, IxCly, a bright yellow solid. If you completely consume 0.678 g of I2 in a reaction with excess Cl2 and produce 1.246 g of IxCly, what is the empirical formula of the compound? A later experiment showed that the molar mass of IxCly was 467 g.mol-1. What is the molecular formula of the compound?
General Chemistry - Standalone book (MindTap Course List)
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Chapter3: Calculations With Chemical Formulas And Equaitons
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Direct reaction of iodine (I2) and chlorine (Cl2) produces an iodine chloride, IxCly, a bright yellow solid. If you completely consume 0.678 g of I2 in a reaction with excess Cl2 and produce 1.246 g of IxCly, what is the empirical formula of the compound? A later experiment showed that the molar mass of IxCly was 467 g.mol-1. What is the molecular formula of the compound?
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