Final answer:
Weighing more zinc chloride than required will not change its empirical formula but will affect the amount of product and the stoichiometry calculations, potentially leading to an incorrect theoretical and percent yield.
Step-by-step explanation:
Using an incorrect mass of zinc chloride, which is greater than the required amount for the experiment, will not change the empirical formula of the compound but will affect the calculations of the chemical amounts. The empirical formula is determined by the mole ratio of the elements in the compound, not the total mass used. However, using more of the compound would yield a greater amount of product, and it may affect the concentration of solutions or the extent of a chemical reaction if the experiment is dependent on specific quantities.
Theoretical yield might be inaccurately calculated if you base it on the larger amount of starting material, leading to a different ratio of products formed compared to the expected results. For instance, in the provided examples, obtaining the empirical formula involves calculating the moles of each element and dividing by the smallest number of moles to get the simplest whole number ratio.
If the mass of zinc chloride would be more than needed, the mass of product obtained could be greater, resulting in an incorrect calculation of percent yield if not adjusted properly. It's crucial to use the precisely weighed amounts in stoichiometry calculations to ensure the experimental results match theoretical predictions.