The equilibrium constant for the reaction: #PCl_5 rightleftharpoons PCl_3 + Cl_2# is 0.0121. A vessel is charged with #PCl_5#, giving an initial pressure of 0.123 atmospheric. How do you calculate the partial pressure of #PCl_3# at equilibrium?
(I have assumed that the quoted equilibrium constant is
Now the given
Given the circumstances of the reaction, I think I am quite justified in assuming that I was given