Question

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g). If initial concentrations are [SO2] = 2.40 M, [O2] = 0.45 M, and [SO3] = 3.60 M, the system is The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g). If initial concentrations are [SO2] = 2.40 M, [O2] = 0.45 M, and [SO3] = 3.60 M, A.the system is not at equilibrium and will shift to the right to achieve an equilibrium state. B.not at equilibrium and will remain in an unequilibrated state. C.at equilibrium. D.not at equilibrium and will shift to the left to achieve an equilibrium state

Answer 1

Option (C) is correct.

The given equation   $2SO_{2(g)} +O_{2(g)}$    ⇄    $2SO_{3(g)}$  is at equilibrium.

Given equation,

                         $2SO_{2(g)} +O_{2(g)}$    ⇄    $2SO_{3(g)}$

and

                   $K_{c} =5.00$   at  1300 K

To determine whether the reaction is at equilibrium or will shift to left or right, determine the Reaction Quotient, which is calculated at any instant of time,

Given,

           $[SO_{2} ]=2.40M$

             $[O_{2} ]=0.45M$

           $[SO_{3} ]=3.60M$

               $Q_{c} =\frac{[SO_{3} ]^2}{[SO_{2} ]^2[O_{2} ]}$

               $Q_{c} =\frac{(3.60)^2}{(2.40)^2(0.45)}$

               $Q_{c} =5$

Since,  

           $K_{c} =5.00$ = $Q_{c}$

The given reaction is at equilibrium.

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