Final answer:
Equivalents for reactants a and b will be in a 1:1 ratio. To improve the yield of the product, calculate the theoretical yield based on the limiting reactant and try to maximize the actual yield by optimizing reaction conditions. The percent yield is obtained by comparing the actual yield with the theoretical yield.
Step-by-step explanation:
In your reaction with reactants a and b at a one molar ratio, their equivalents will also be in a one-to-one ratio, meaning you'll use equimolar amounts of a and b to attain complete reaction without any left-over reactant. To improve the yield of the product, you'd typically aim to maximize the actual yield relative to the theoretical yield using a variety of methods, such as optimizing reaction conditions or using catalysts.
First, you'll want to determine the limiting reactant since this will dictate the maximum amount of product that can be formed; this is done by calculating the amount of product that can be formed from the given amount of each reactant and identifying the smallest amount. Once you've found your limiting reactant, you can calculate the theoretical yield based on the balanced equation's stoichiometry.
To improve the percent yield, one can focus on reducing by-products, increasing reaction completeness, or enhancing product recovery. Sometimes changing reaction conditions such as temperature, pressure, or concentration can help, as might the use of catalysts or optimizing the reaction timeline.
The percent yield is calculated by dividing the actual yield by the theoretical yield and multiplying by 100. Maximizing the percent yield will involve meticulous control of reaction parameters to ensure that you approach as close to the theoretical yield as possible.