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Consider the following system at equilibrium where $H=198kJ,$ and $K_c=0\mathrm{.}0290,$ at $1150K$ :

$2S{O}_3(g)2S{O}_2(g)+O_2(g)$

When $0\mathrm{.}37$ moles of $S{O}_2(g)$ are removed from the equilibrium system at constant temperature:

The value of $K_c$

increases

decreases

remains the same

The value of $Q_c$

is greater than $K_c$

is equal to $K_c$

is less than $K_c$

The reaction must

run in the forward direction to reestablish equilibrium

run in the reverse direction to reestablish equilibrium

remain in the current position, since it is already at equilibrium

The concentration of $S{O}_2$ will

increase

decrease

remain the same