The equilibrium mixture for
`2SO_(2)(g) +O_(2)(g) hArr 2SO_(3)(g)`
present in `1 L` vessel at `600^(@)C` contains `0.50, 0.12`, and `5.0` moles of `SO_(2), O_(2)`, and `SO_(3)` respectively.
a. Calculate `K_(c)` for the given change at `600^(@)C`.
b. Also calculate `K_(p)`.
c. How many moles of `O_(2)` must be forced into the equilibrium vessel at `600^(@)C` in order to increase the concentration of `SO_(3)` to `5.2` mol?

Answer

A, B, C

Explanation

`{:(,2SO_(2),+,O_(2),hArr,2SO_(3)),("moles at",0.5,,0.12,,5.0),("equilibrium",,,,,),("Volume"=1 L,,,,,):}`
a. `K_(c)=([SO_(3)]^(2))/([SO_(2)]^(2)[O_(2)])=((5)^(2))/((0.5)^(2)(0.12))`
`K_(c)=833.33`
b. `K_(P)=K_(C)(RT)^(Deltan)=833.33xx(0.0821xx873)^(-1)`
`=11.62 ("atm")^(-1)`