Now, I'm not going to go into much detail about this guy because I just want you to be aware that this guy exists. Now if reactants and products are both in the gas state, we can still use the equilibrium constant and the expression equilibrium constant. But now we have to incorporate the partial pressures of our gases. For example, suppose we have the following reaction in which gas A react with gas B to produce gas C and gas D, where it lowercase A-B-C and D are the coefficients of each respective atom that represent the moles of each atom. For example, lowercase a number of moles of A gas reacts with B number of moles of B gas produces C number of moles of C gas and B number of moles of D gas. Now our equilibrium constant for this gaseous reaction is the following our equilibrium constant KP is equal to the partial pressure of our C of our gas product C to the C power.