Question

2cocl₂·6h₂o + 2 nh₄cl + 8 nh₃ h₂o₂ → 2 [co(nh₃)₅h₂o]cl₃ +12 h₂o

for this reaction 3.2 g of cocl₂·6h₂o reacts with 1.2 g of nh₄cl, 3.5 ml of 15 m nh₄oh and 2.5 ml of 10.% h₂o₂. the h₂o₂ is 10.% by mass and the density of the h₂o₂ is 1.0 g/ml and the moles of nh₃ is calculated from the moles of nh₄oh added (nh₃(aq) = nh₄oh (aq)). assume the reaction goes to completion.
From the information given, determine the limiting reagent.

Answer 1

To find the limiting reagent in the reaction, calculate the moles of each reactant using their provided masses, concentrations, and densities, and compare these to the stoichiometric coefficients in the balanced equation. The reactant that produces the least amount of product is the limiting reagent.

Step-by-step explanation:

In this chemistry problem, we are tasked with determining the limiting reagent for the given reaction. To find the limiting reagent, we must first calculate the moles of each reactant based on the given masses and concentrations. Beginning with CoCl₂·6H₂O, we use its molar mass to convert the provided 3.2 g to moles. Similarly, we convert the 1.2 g of NH₄Cl into moles using its molar mass.

For NH₃, it is derived from NH₄OH in solution, so we use the volume (in liters) and molarity to find the moles of NH₄OH, which are equivalent to the moles of NH₃ as per the question's information. Lastly, the volume of H₂O₂ is multiplied by its density to get the mass, and then we calculate the mass of H₂O₂ present in the solution using the percentage given. This mass is then converted to moles using the molar mass of H₂O₂.

Once all mole quantities are available, we compare them to the stoichiometric coefficients in the balanced equation to identify the limiting reagent. The one that provides the least amount of product according to the stoichiometric ratio is the limiting reagent. This approach of reactant-to-product mole comparison is essential in stoichiometry to determine the extent of chemical reactions.