Following equilibria are established in three different equal volume containers.

Reaction I: $X_{2\left(g\right)}+Y{O}_{2\left(g\right)}\rightleftharpoons X_2{O}_{\left(g\right)}+Y{O}_{\left(g\right)}; K_{eq}$  at  $2000K=4$
Reaction II: $2X_2{O}_{\left(g\right)}\rightleftharpoons 2{X_2}_{\left(g\right)}+{O_2}_{\left(g\right)}; K_{eq}$ at $2000K=5\times {10}^{-10}$
Reaction III: $2Y{O}_{\left(g\right)}+O_{2\left(g\right)}\rightleftharpoons 2Y{O_2}_{\left(g\right)}; K_{eq}$ at $1000K=2.5\times {10}^{22}$
Which of the following statements is/are CORRECT?

In reaction I, equilibrium amount of $Y{O}_{\left(g\right)}$ can be increased by increasing the  volume of container at constant temperature

In reaction III, equilibrium amount of $Y{O}_{\left(g\right)}$ can be increased by decreasing the  pressure at constant temperature.

In reaction II, addition of Helium gas at constant volume and temperature increases  the equilibrium amount of $O_{2\left(g\right).}$

In reaction III, the forward reaction must be exothermic.