Final answer:
This question discusses evaluating the effect of doubling a reactant concentration on reaction rate according to the rate law, the identification of limiting reactants through stoichiometry, and the use of the ideal gas law in analyzing chemical reactions.
Step-by-step explanation:
The question involves the determination of reaction rates and the effects of concentration changes on these rates in Chemistry, particularly within the context of the rate law, stoichiometry, and the ideal gas law. Evaluating the limit mentioned in the question seems to be unrelated to these chemical concepts and might be a typographical error, as limits pertain to Mathematics rather than Chemistry. However, assuming the student meant to inquire about the effect of changing reactant concentrations on the reaction rate, one would use the mathematical relationships of the rate law. To determine the effect of doubling the concentration of a single species, one should identify the order of the reaction with respect to that species in the rate law. If the concentration of a reactant is doubled and it is a first-order reactant, the rate of the reaction will also double. If it is second-order with respect to that reactant, the rate will quadruple, and so on.
When considering stoichiometry and limiting reactants, it is critical to balance the chemical equation, convert given reactant amounts to moles, and compare these to the stoichiometric ratios in the balanced equation to identify the limiting reactant. The limiting reactant then determines the maximum amount of product that can be formed.
The ideal gas law can be used to relate the moles of gas to its pressure, volume, and temperature, which is helpful in understanding and predicting the behavior of gases in chemical reactions.