Question

he 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] = 6.00 M, [O2] = 0.45 M, and [SO3] = 9.00 M, the system isnot at equilibrium and will shift to the right to achieve an equilibrium state.not at equilibrium and will shift to the left to achieve an equilibrium state.at equilibrium.not at equilibrium and will remain in an unequilibrated state.

Answer 1

Answer:

The system is at equilibrium

Explanation:

Let's consider the following reversible reaction.

2 SO₂(g) + O₂(g) ⇄ 2 SO₃(g)

To determine whether a reaction is at equilibrium or not, we have to calculate the reaction quotient (Q).

$Q=\frac{[SO_{3}]^{2}}{[SO_{2}]^{2}.[O_{2}]} =\frac{(9.00)^{2} }{(6.00)^{2}\times 0.45} =5.0$

Since Q = K (equilibrium constant), regardless of the significant figures, the system is at equilibrium.