Chemistry - Mole Concept Question with Solution | TestHub

Let $x$ be the moles of ICl formed and $y$ be the moles of ICl₃ formed.

The balanced chemical equations for the formation of ICl and ICl₃ from I₂ and Cl₂ are:

1. $\frac{1}{2}{I}_2+\frac{1}{2}C{l}_2⟶ICl$

2. $\frac{1}{2}{I}_2+\frac{3}{2}C{l}_2⟶IC{l}_3$

Alternatively, we can consider the overall reaction:

$I_2+aC{l}_2⟶xICl+yIC{l}_3$

Balancing I atoms: $2=x+y$ (Equation 1)

Balancing Cl atoms: $2a=x+3y$

From the given moles, we have 0.1 mol of I₂ and 0.2 mol of Cl₂.

So, for I atoms: $2\times 0.1=x+y⟹0.2=x+y$ (This is Equation 1)

For Cl atoms: $2\times 0.2=x+3y⟹0.4=x+3y$ (Equation 2)

Now we solve the system of equations:

1) $x+y=0.2$

2) $x+3y=0.4$

Subtract Equation 1 from Equation 2:

$(x+3y)-(x+y)=0.4-0.2$

$2y=0.2$

$y=0.1$ mol

Substitute $y=0.1$ into Equation 1:

$x+0.1=0.2$

$x=0.1$ mol

So, moles of ICl ($x$) = 0.1 mol

Moles of ICl₃ ($y$) = 0.1 mol

The ratio of moles of ICl : ICl₃ is $0.1:0.1$, which simplifies to $1:1$.

The final answer is $\boxed{1:1}$.