For the exothermic gas-phase reaction 2 SO 2(g) + O 2(g) rightleftharpoons 2 SO 3(g) with Delta H < 0, which set of condition changes will shift equilibrium toward products?

Decreasing temperature and increasing system pressure

Increasing temperature and decreasing system pressure

Increasing temperature and increasing system pressure

Decreasing temperature and decreasing system pressure

For the exothermic gas-phase reaction $2 SO_{2} (g) + O_{2} (g) ⇌ 2 SO_{3} (g)$ with $Δ H < 0$ , which set of condition changes will shift equilibrium toward products?

Free questions with an explanation for every one, and full timed SIMAK UI mock tests.