Calculate `K_p` from `K_c`: The equilibrium constant, `K_c`, for the reaction
`N_2O_4(g) hArr 2NO_2(g)`
is `3.64xx10^-3` at `25^@C`. What is the value of `K_p` at this temperature?

Explanation

Strategy: Use Eq. to calculate `K_p` from `K_c` and use chemical equation to find `Deltan_g`, i.e., the change in the number of moles of gas as the reaction proceeds from left to right.
Solution: From Eq. , we write
`K_p=K_c(RT)^(Deltan_g)`
Since `K_c=3.64xx10^-3`, `R=0.081 L` atm `K^(-1)mol^(-1)`, `T=298K`, and `Deltan_g=(2-1)=1`, we have
`K_p=(3.64xx10^-3)(0.0821)(298)`
`=0.089`