Final answer:
The question involves solving a chemical equilibrium problem for the reaction between hydrogen and fluorine to form hydrogen fluoride. The initial partial pressures are given, and the equilibrium constant at 298 K is known. An ICE table would be used alongside the equilibrium constant expression to find the equilibrium partial pressures.
Step-by-step explanation:
The question pertains to a chemical equilibrium problem involving the reaction 2F(g) + H₂(g) → 2HF (g) at 298 K. In this reaction, hydrogen (H₂) and fluorine (F₂) gases react to form hydrogen fluoride (HF(g)). The equilibrium constant for the reaction, Kp, is 5.07 × 10⁴. To calculate the partial pressures at equilibrium, we can set up an ICE (Initial, Change, Equilibrium) table and apply the equilibrium constant expression.
Starting with the initial partial pressures of H₂ and F₂, 0.03500 atm and 0.06800 atm respectively, we let 'x' represent the change in partial pressure due to reaction. At equilibrium, the partial pressure of H₂ will be 0.03500 - x atm, that of F₂ will be 0.06800 - 2x atm, and that of HF(g) will be 2x atm. By substituting these expressions into the equilibrium constant formula Kp = [HF]2/([H₂][F₂]), and solving for 'x', we would find the equilibrium partial pressures of each gas.
Although we do not provide the calculations here, it is important to understand that this approach utilizes the stoichiometry of the balanced chemical equation, knowledge of equilibrium expressions, and algebraic techniques to solve for the unknown 'x'. From 'x', we can determine the final partial pressures of each gas involved in the equilibrium.