The equilibrium concentration of CO₂ when a mixture that is
1.5M in CO and 1.2M in CO₂ are mixed to make 1.0L of the solution is 2.43 M.
[tex]$\begin{aligned} k_{c} &=\frac{\left[\mathrm{CO}_{2}\right]}{[\mathrm{C0}]}=\frac{(1.2+x)}{(1.5-x)} \\ \therefore \quad 9.0 &=\frac{(1.2+x)}{\left(1.5^{-\pi} x\right)} \\ \text { or, } 9 \times 1.5 &-9 x=1.2+x \end{aligned}$[/tex]
or, [tex]$\begin{aligned} 10 x &=13.5-1.2=12.3 \\ \text { or, } x &=1.23 \end{aligned}$[/tex]
[tex]\therefore \begin{aligned}\therefore eq^{n}{com}^{n} \text { of } \mathrm{CO}_{2} &=(1.2+\lambda) \mathrm{M} \\&=(1.2+1.23) \\&=2.43 \mathrm{M} .\end{aligned}[/tex]
A chemical reaction is considered to be in a state of chemical equilibrium when both the reactants and the products are in a concentration that does not change over time anymore. The forward response rate and the backward reaction rate are equal in this condition.
The equilibrium will adjust to minimise the impact of a change in a substance's concentration. Reactant concentration will drop if a reactant's concentration is raised because the equilibrium will change in favour of the reaction that utilises the reactants.
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