Chemistry: : Starting with 0.3500 mol CO(g) and 0.05500 mol COCl2(g) in a 3.050-L flask at 668 K, how many moles of Cl2(g) will be present at equilibrium

1 and 2Explanation:Hopefully this helps!...

: Starting with 0.3500 mol CO(g) and 0.05500 mol - id035000055007061467, issaaamiaaa15

christheicebear

30.01.2022

The number of moles of Cl₂ present at equilibrium is 3.94x10⁻⁴ moles.

Explanation:

The reaction is:

CO(g) + Cl₂(g) ⇄ COCl₂(g)

The equilibrium constant of the above reaction is:

K = 1.2x10³

To find the moles of Cl₂ present at equilibrium, let's evaluate the reverse reaction:

COCl₂(g) ⇄ CO(g) + Cl₂(g)

The equilibrium constant for the reverse reaction is:

$K_{r} = \frac{1}{1.2 \cdot 10^{3}} = 8.3 \cdot 10^{-4}$

Now, we need to calculate the concentration of CO and COCl₂:

$C_{CO} = \frac{\eta_{CO}}{V} = \frac{0.3500 moles}{3.050 L} = 0.115 M$

$C_{COCl_{2}} = \frac{\eta_{COCl_{2}}}{V} = \frac{0.05500 moles}{3.050 L} = 0.018 M$

Now, from the reaction we have:

COCl₂(g) ⇄ CO(g) + Cl₂(g)

0.018 - x 0.115+x x

The concentration of Cl₂ is:

$K_{r} = \frac{[CO][Cl_{2}]}{[COCl_{2}]}$

$8.3 \cdot 10^{-4} = \frac{(0.115 + x)(x)}{0.018 - x}$

$8.3 \cdot 10^{-4}*(0.018 - x) - (0.115 + x)(x) = 0$

By solving the above equation for x we have:

x = 1.29x10⁻⁴ M = [Cl₂]

Finally, the number of moles of Cl₂ present at equilibrium is:

$\eta_{Cl_{2}} = C_{Cl_{2}}*V = 1.29 \cdot 10^{-4} mol/L*3.050 L = 3.94 \cdot 10^{-4} moles$

Therefore, the number of moles of Cl₂ present at equilibrium is 3.94x10⁻⁴ moles.

I hope it helps you!

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