Explanation:

Step 1: Balanced Chemical Equation
The balanced chemical equation for the given reaction is:
2SO2(g) + O2(g) → 2SO3(g)

Step 2: Calculation of Total Moles of Gases
Total moles of gases present in the mixture = moles of SO2 + moles of O2 = 10 + 4 = 14 moles

Step 3: Calculation of Partial Pressures
Partial pressure of SO2 in the mixture = moles of SO2 / total moles of gases x total pressure = 10/14 x P
Partial pressure of O2 in the mixture = moles of O2 / total moles of gases x total pressure = 4/14 x P
where P is the total pressure of the mixture.

Step 4: Calculation of Equilibrium Constant
The equilibrium constant (Kc) for the given reaction at a given temperature is calculated by using the formula:
Kc = ([SO3]^2 / [SO2]^2 [O2])
where [SO3], [SO2], and [O2] are the equilibrium concentrations of the respective gases.

Step 5: Calculation of Equilibrium Concentrations
The equilibrium concentrations of the gases can be calculated by using the initial moles of gases, the volume of the container, and the stoichiometry of the reaction.

Step 6: Calculation of Equilibrium Partial Pressures
The equilibrium partial pressures of the gases can be calculated by using the equilibrium concentrations of the gases and the total pressure of the mixture.

Step 7: Comparison of Equilibrium Constants
The calculated equilibrium constant is compared with the experimental equilibrium constant to determine the extent of the reaction.

Step 8: Explanation of the Reaction
The reaction between SO2 and O2 in the presence of a platinum catalyst produces SO3. The platinum catalyst provides a surface for the reaction to occur and lowers the activation energy required for the reaction to take place. The reaction is an exothermic reaction, which means that it releases heat. The extent of the reaction depends on the initial concentrations of the reactants, the temperature, and the pressure of the mixture.

When so2 react with o2 it's produces so3 and heat