Grade 11Physical Chemistry

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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Sanskar patwa

9 Years agoGrade 11

2 Answers

varun

9 Years ago

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

THANK YOU

Yash Chourasiya

6 Years ago

Hello Student

I₂+ 2Cl₂→ ICl + ICl₃
Molar mass of I₂ = 253.80
Molar mass of Cl₂ = 70.9
Moles of I₂ used = 25.4/253.80 = 0.1 moles ofI₂
Moles of Cl₂ used = 14.2/70.9 = 0.2 moles ofCl₂

Since the stoichiometry indicates that each mole of I₂ reacts with 2 moles of Cl₂ togive 1 mole each of ICl and ICl₃.
Chlorine is limiting reagent, in this case, hence 0.2-mole chlorine will react with 0.1 moles of iodine to form 0.1 mole each of the product.

So option (A) is correct.

I hope this answer will help you.