Question

254 g of Iodine and 142 g of Chlorine are made to react completely to give a mixture of $ICl$ and $IC{l}_3$. Moles of each product formed are:
(i) 0.1 mole $ICl$ and 0.1 mole $IC{l}_3$
(ii) 1.0 mole $ICl$ and 1.0 mole $IC{l}_3$
(iii) 0.5 mole $ICl$ and 0.1 mole $IC{l}_3$
(iv) 1.5 mole $ICl$ and 1.0 mole $IC{l}_3$

Answer 1

Hint: Compounds always react in the ratio of stoichiometric coefficients of the completely balanced reaction. This principle is based on the conservation of mass that states that total mass of reactant will always be equal to total mass of product. Therefore total moles of each type of atom will also be the same on both sides.

Complete step by step answer:
$I_2+2C{l}_2\to ICl+IC{l}_3$ Iodine and chlorine will react according to following reaction:
$I_2+2C{l}_2\to ICl+IC{l}_3$
1 mole iodine is reacting with 2 mole chlorine to form 1 mole $ICl$ and 1 mole $IC{l}_3$
So iodine and chlorine are reacting in the molar ratio of 1 : 2
Number of moles= ${\displaystyle \frac{givenmass}{molarmass}}$
As given in the question:
Gram molecular weight of Iodine ($I_2$) = 254 g
Gram molecular weight of Chlorine ($C{l}_2$) = 142 g
Number of moles of iodine = ${\displaystyle \frac{254}{254}}$
Number of moles of iodine= 1 mole
Number of moles of chlorine = ${\displaystyle \frac{142}{71}}$
Number of moles of chlorine= 2 mole
So here chlorine and iodine available in the ratio of 1:2 therefore limiting reagent concept will not be applicable and any reactant can decide the yield of the product.
- As according to reaction stoichiometry 1 mole iodine is producing 1 mole $ICl$ and 1 mole $IC{l}_3$.
Therefore, $ICl$ obtained = 1 mole
 $IC{l}_3$ obtained = 1 mole

Additional Information :Iodine is a lustrous, non-metallic, purple-black solid with atomic number 53 and electronegativity of 2.66. Chlorine is a gas with atomic number 15 and electronegativity of 3.16.

Note: The limiting reagent is the reactant that is completely used up in a reaction, and thus determines when the reaction stops therefore determines yield of product. Here as both the reactants are reacting completely, therefore both get completely used up together and no one is limiting reagent in this reaction.