The following equilibrium concentrations were measured at 800K:[SO2]=3.0×10−3 M; [O2]=3.5×10−3 M; [SO3]=5.0×103 M Calculate the equilibrium constant at 800 K for the chemical reaction in equilibrium for both directions.2SO2(g)+O2(g)⇌2SO3(g)(Kc is the equilibrium constant for the forward reaction and K′c is the equilibrium constant for the backward reaction)

The following equilibrium concentrations were measured at 800K:[SO2]=3

1.	The following equilibrium concentrations were measured at 800K:[SO2]=3.0×10−3 M; [O2]=3.5×10−3 M; [SO3]=5.0×103 M Calculate the equilibrium constant at 800 K for the chemical reaction in equilibrium for both directions.2SO2(g)+O2(g)⇌2SO3(g)(Kc is the equilibrium constant for the forward reaction and K′c is the equilibrium constant for the backward reaction)
Answer» The following equilibrium concentrations were measured at $800 K : [S O_{2}] = 3.0 \times 10^{- 3} M; [O_{2}] = 3.5 \times 10^{- 3} M; [S O_{3}] = 5.0 \times 10^{3} M$ Calculate the equilibrium constant at $800 K$ for the chemical reaction in equilibrium for both directions. $2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$ ( $K_{c}$ is the equilibrium constant for the forward reaction and $K_{c}^{^{'}}$ is the equilibrium constant for the backward reaction)