Molecular hydrogen (H₂) is heated in a nuclear rocket chamber to a temperature of 3000 K. The equilibrium constant for the hydrogen dissociation reaction H2 -> 2H at this temperature is Kp=(P_H)² / (P_H2) = 0.03; where P is in atmospheres. If the chamber pressure is 10 atm, calculate the mole fractions of H₂ and H.

This is a propulsion question, please only answer if you know what you're doing

Molecular hydrogen (H2) is heated in a nuclear rocket chamber to a temperature of 3000K. The equilibrium constant for the hydrogen dissociation reaction H22H at this temperature is Kp=(pH)2/(pH2)=0.03, where p is in atmospheres. If the chamber pressure is 10atm, calculate the mole fractions of H2 and H