At `700 K`, the equilibrium constant `K_(p)` for the reaction `2SO_(3)(g)hArr2SO_(2)(g)+O_(2)(g)` is `1.80xx10^(-3) kPa`. What is the numerical value of `K_(c )` in moles per litre for this reaction at the same temperature?

At `700 K`, the equilibrium constant `K_(p)` for the reaction `2SO_(3)

1.	At `700 K`, the equilibrium constant `K_(p)` for the reaction `2SO_(3)(g)hArr2SO_(2)(g)+O_(2)(g)` is `1.80xx10^(-3) kPa`. What is the numerical value of `K_(c )` in moles per litre for this reaction at the same temperature?
Answer» For the reaction `2SO_(3)(g)hArr2SO_(2)(g)+O_(2)(g)` Here `n_(p)=3 "mol", n_(r)=2 "mol"` `:.Deltan=n_(p)-n_(r)=3-2=1 "mole"` `K_(p)=1.80xx10^(-3) kPa` `R=8.314 J K^(-1) "mol"^(-1)` `T=700 K` Using the relation, `K_(p)=K_(c )(RT)^(Deltan)` `K_(c )=K_(p)/(RT)=(1.80xx10^(-3))/(8.314xx700)=3.09xx10^(-7) "mol" L^(-1)`

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At `700 K`, the equilibrium constant `K_(p)` for the reaction `2SO_(3)(g)hArr2SO_(2)(g)+O_(2)(g)` is `1.80xx10^(-3) kPa`. What is the numerical value of `K_(c )` in moles per litre for this reaction at the same temperature?

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