Consider the equilibrium reaction: 2HCl_((g))leftharpoons H_(2(g))+Cl_(2(g)) . Initially, a container contains only HCl gas at a partial pressure of 0,8 atm. If the equilibrium constant (Kp) for the reaction is 0,04 . what is the partial pressure of Cl_(2) at equilibrium __ A. 0,4 atm B. 0,2 atm C.0,1 atm D.0,8 atm E. 0,4 atm

To find the partial pressure of at equilibrium, we need to set up an ICE table (Initial, Change, Equilibrium) and use the equilibrium constant expression.The balanced chemical equation is: Let's denote the initial partial pressure of as atm.At equilibrium, let the change in pressure for be , for be , and for be .So, the equilibrium pressures will be:- - - The equilibrium constant expression for this reaction is: Given , we substitute the equilibrium pressures into the expression: Now, solve for : This is a quadratic equation in the form . Solve it using the quadratic formula : Taking the positive root (since pressure cannot be negative): Thus, the partial pressure of at equilibrium is approximately atm.Therefore, the correct answer is:C. 0.1 atm