Final answer:
In order to find the equilibrium partial pressure of H₂, write out the equilibrium equation and plug in the given values. Then, solve for the unknown to obtain the pressure. Solving the equation might require mathematical software or calculators that can find roots.
Step-by-step explanation:
The chemical equilibrium equation for the given reaction is Kp = (P(H₂) * P(F₂)) / (P(HF)²). We are given that Kp = 2.76 and P(HF) = 0.0670 atm at the start. Since the equilibrium constant Kp for the reaction is greater than 1, the reaction will proceed in the forward direction where 2 moles of HF dissociate into 1 mole each of H₂ and F₂.
Let's assume that x atm of HF dissociates at equilibrium. Therefore, the equilibrium partial pressures of H₂ and F₂ are both x, and the equilibrium partial pressure of HF is 0.0670 - 2x. Plug these values into the equilibrium equation and solve it: 2.76 = x² / (0.0670 - 2x)². Solve this equation for x to find the equilibrium pressure of H₂. In physical chemistry, solving such equations usually involves the use of mathematical software or calculators with root finding abilities.
Learn more about Chemical Equilibrium