Final answer:
The reaction in question is 2SO2(g) + O2(g) → 2SO3(g), and the reaction rate can be calculated based on the stoichiometry of the equation, with negative rates for reactants and positive rates for products. Equilibrium constants are also related to the temperature of the system, changing based on whether the reaction is exothermic or endothermic.
Step-by-step explanation:
The chemical reaction in the initial rate data is 2SO2(g) + O2(g) → 2SO3(g). This balanced equation indicates that two moles of sulfur dioxide gas (SO2) react with one mole of oxygen gas (O2) to produce two moles of sulfur trioxide gas (SO3).
To calculate the reaction rate of SO2 with O2 to produce SO3, the rate expressions are based on the stoichiometry of the balanced chemical equation. For the reactants, the rates are negative because their concentrations decrease as the reaction proceeds. For the products, the rates are positive. The rate of disappearance of SO2 is twice the rate of disappearance of O2, as per the balanced equation. Similarly, the rate of formation of SO3 is equal to the rate of disappearance of SO2 because two moles of SO3 are formed for every two moles of SO2 consumed.
Also, understanding the relationship between equilibrium constants and temperature can be determined by applying Le Châtelier's principle. If the reaction is exothermic, then increasing the temperature would decrease the equilibrium constant as the system shifts to favor the reactants to absorb excess heat.