A sample of `CaCO_(3)(s)` is introduced into a sealed container of volume `0.654 L` and heated to `1000 K` until equilibrium is reached. The equilibrium constant for the reaction `CaCO_(3)(s)hArrCaO(s)+CO_(2)(g),` is `3.9xx10^(-2)` atm at this temperature. Calculate the mass of `CaO` present at equilibrium.

A sample of `CaCO_(3)(s)` is introduced into a sealed container of vol

1.	A sample of `CaCO_(3)(s)` is introduced into a sealed container of volume `0.654 L` and heated to `1000 K` until equilibrium is reached. The equilibrium constant for the reaction `CaCO_(3)(s)hArrCaO(s)+CO_(2)(g),` is `3.9xx10^(-2)` atm at this temperature. Calculate the mass of `CaO` present at equilibrium.
Answer» `CaCO_(3)(s)(s)hArrCaCO_(2)(g)` `K_(p)=p_(CO_(2))=3.9xx10^(-2)` Let the number of "moles" of `CO_(2)` be formed `=n` `n=(p_(CO_(2))xxV)/(RT)=(3.9xx10^(-2)xx0.654)/(0.082xx1000)=3.11xx10^(-4) "mol"` The amount of `CaO(s)` formed will also be `=3.11xx10^(-4) "mol"` Hence, the mass of `CaO` formed `=3.11xx10^(-4)xx56` `=0.0174 g`

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