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Class 11th Chemistry1) 25.4g of iodine and 12.2 g of chlorine are made to react completely to yield a mixture of ICl and ICl3. Calculate the ratio of the miles of ICl and ICl3

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25.4 g of iodine and 14.2 g of chlorine are made to react completely to yield a mixture of ICL and ICL3 . CALCULATE the no. Of moles of ICL and ICL3 formed.

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It is based on principle of POAC

see given that I2 + 2CL2 gives ICL + ICL3.

Now we have molar mass of I2 =127x2=254

Molar mass of Cl2=35.5x2=71

So,,moles of I2 used in the reaction =given mass/molar mass =25.4/254=0.1 moles of I2

Moles of Cl2 used in the reaction is =14.2/71=0.2 moles of Cl2

so and therefore from the reaction we see that 1 mol of I2 react with 2 moles of Cl2 to give one mole of each ICL and ICL3

Interpreting the same data with the same data with the given sample we can conclude that 0.2 mol of Cl2 reacts with 0.1 mol of iodine to give 0.1 mol of each ICL and ICL3


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