Step-by-step explanation:
the reaction being referred to is the one where sulfur dioxide (SO2) and oxygen (O2) react to form sulfur trioxide (SO3) according to the following balanced equation:
2 SO2(g) + O2(g) ⇌ 2 SO3(g)
If the equilibrium is established by beginning with equal numbers of moles of SO2 and O2, i.e., if the initial molar amounts of SO2 and O2 are the same, then we can conclude the following at equilibrium:
The rate of the forward reaction (2 SO2(g) + O2(g) → 2 SO3(g)) is equal to the rate of the reverse reaction (2 SO3(g) → 2 SO2(g) + O2(g)).
The concentrations of SO2, O2, and SO3 will remain constant over time.
The amounts of SO2, O2, and SO3 present at equilibrium will depend on the temperature, pressure, and other conditions of the system.
The value of the equilibrium constant (Kc) for the reaction will have a specific numerical value at equilibrium, which will depend on the temperature and other conditions of the system.
The value of the reaction quotient (Qc) for the reaction will be equal to the equilibrium constant (Kc) at equilibrium, indicating that the system is at equilibrium
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