25.4 g of iodine and 7.1 g chlorine are made to react to give a mixture of ICl and $I C l_{3}$ . Number of moles of ICl and $I C l_{3}$ formed are respectively ?

25.4 g

I_{2}

and

14.2 g

C l_{2}

are made to react completely to yield a mixture of

I C l

and

I C l_{3}

. Calculate the number of moles of

I C l

and

I C l_{3}

. (Given: Molar mass of

I

127

g / m o l

)

25.4 g of

I_{2}

and 14.2 of

C l_{2}

are made to react completely to form

I C l

and

{I C l}_{3}

. Determine

(i) Limiting reagent(ii) No. of moles of

I C l

and

{I C l}_{3}

formed.

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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 ratio of moles of ICl and ICl3.

The correct option is A 1:1Balanced reaction is given below: I2+2Cl2→ICl+ICl3Stoichiometry coefficient of ICl and ICl3 are equal. So, every time equal number of moles of ICl and ICl3 will be produced irrespective of amount of reactant used.So, ratio of moles of ICl and ICl3 produced is 1:1.

$25.4$ g of iodine and $14.2$ g of chlorine are made to react completely to yield a mixture of $I C l$ and ${I C l}_{3}$ . Calculate the ratio of moles of $I C l$ and ${I C l}_{3}$ .