Consider the following hypothetical chemical reaction: 2A + B ⟶ C + 3D The reaction was studied under various conditions, and it was found that the rate of formation of product C was inversely proportional to the concentration of reactant B. Additionally, it was observed that doubling the initial concentration of reactant A resulted in a fourfold increase in the rate of formation of product C. Based on this information, answer the following questions: What is the order of the reaction with respect to reactant A? What is the order of the reaction with respect to reactant B? What is the overall order of the reaction? Write the rate law expression for this reaction. If the initial concentration of reactant A is tripled while keeping the concentration of reactant B constant, what will be the effect on the rate of formation of product C?

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