What is the maximum mass of H2O that can be produced by combining 85.0 g of each reactant?
Do you have any particular reactants in mind?
To find the maximum mass of H2O that can be produced, we first need to determine which reactant is limiting, i.e., the reactant that will be completely consumed and therefore determine the amount of product formed.
Given that we have 85.0 g of each reactant, we can calculate the number of moles for each reactant using their molar masses. The molar mass of H2O is 18.015 g/mol.
First, let's find the number of moles of each reactant:
Number of moles of reactant 1 (let's call it A):
moles of A = mass of A / molar mass of A
Number of moles of reactant 2 (let's call it B):
moles of B = mass of B / molar mass of B
In this case, both reactants are H2O, so the molar masses are the same. Therefore, both moles of A and B will be equal:
moles of A = moles of B = mass of A / molar mass of A
moles of A = moles of B = 85.0 g / 18.015 g/mol
Now, we need to determine the stoichiometry of the reaction to find the molar ratio between the reactants and the product. The balanced equation is required for this step, if it is given.
Once we have the molar ratio, we can compare the moles of reactants to see which reacts in a limiting manner - i.e., which has a smaller number of moles to react completely with the other reactant.
Finally, we can calculate the mass of H2O produced using the moles of the limiting reactant and its molar mass:
mass of H2O = moles of limiting reactant × molar mass of H2O
By following these steps, you can determine the maximum mass of H2O that can be produced.