Answer:
The maximum number of moles of H2 that can be produced by the reaction of 3.00 mol of Ni with 4.50 mol of HCl is 2.25 moles.
Explanation:
You know you have 3.00 mol of Ni and 4.50 mol of HCl, so you must first determine the limiting reagent.
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
To determine the limiting reagent, it is possible to use the reaction stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), and the amount of moles of each compound given as data. You can use a simple rule of three as follows: if by stoichiometry one mole of Ni reacts with 2 moles of HCl, how much moles of HCl will be needed if 3.00 moles of Ni react?
moles of HCl= 6
But 6 moles of O2 are not available, 4.50 moles are available. Since you have less moles than you need to react with 3.00 moles of Ni, hydrochloric acid HCl will be the limiting reagent.
Then, taking into account that you must work with the acid because it is the limiting reagent and using the amount of moles you have as data, it is possible to determine the amount of moles of H2 produced by another rule of three: if by stoichiometry 2 moles of HCl produce 1 mole of H2, how many moles of H2 will be formed if 4.5 moles of HCl react?
moles of CO2=2.25 moles
Then, the maximum number of moles of H2 that can be produced by the reaction of 3.00 mol of Ni with 4.50 mol of HCl is 2.25 moles.
