Final answer:
The student's question pertains to chemical equilibrium and the calculation of partial pressures. Without detailed reaction conditions, it's not possible to provide the exact pressure of CO formed. Dalton's Law and the ideal gas law are key to solving these types of problems.
Step-by-step explanation:
The student's question seems to be based on a reaction between carbon monoxide (CO) and a solid carbon (C) to produce carbon dioxide (CO₂), which is a typical chemistry problem related to the calculation of partial pressures and equilibrium constants.
It is essential to use the principles of chemical equilibrium and Dalton's Law (partial pressures) to solve such problems. Dalton's Law states that the total pressure in a mixture of gases is the sum of the individual partial pressures of each gas. To calculate the pressure of CO after the reaction is complete, the student must find the change in partial pressure due to the reaction, taking into account the mole ratio between reactants and products. Without the exact reaction conditions or equilibrium constant, it's not possible to provide a precise answer to the student's question. The percentages for dissociation of CO₂ would typically be obtained from the starting and equilibrium conditions using stoichiometry and the ideal gas law.