Al(OH)3(s) + HCl(aq) AlCl3(aq) + H2O(l)
How many moles of HCl are required to react with 0.470 g of Al(OH)3 in the above unbalanced reaction? Use at least as many significant figures in your molar masses as in the data given.
mol HCl
What mass of HCl is required?
How many moles of H2O are produced?
What mass of H2O is produced?
To answer these questions, we need to use the balanced equation provided and apply stoichiometry.
1. Let's start by finding the mole ratio between HCl and Al(OH)3. From the balanced equation, we can see that the ratio is 3 moles of HCl to 1 mole of Al(OH)3.
2. To find the number of moles of HCl, we can use the molar mass of Al(OH)3 and the given mass of Al(OH)3. The molar mass of Al(OH)3 is calculated as:
(1 atom of Al x atomic mass of Al) + (3 atoms of O x atomic mass of O) + (3 atoms of H x atomic mass of H)
Next, we calculate the moles of Al(OH)3:
moles of Al(OH)3 = given mass of Al(OH)3 in grams / molar mass of Al(OH)3
3. Using the mole ratio, we can determine the moles of HCl:
moles of HCl = moles of Al(OH)3 * (3 moles of HCl / 1 mole of Al(OH)3)
4. To find the mass of HCl required, we multiply the moles of HCl by its molar mass:
mass of HCl = moles of HCl * molar mass of HCl
5. To determine the moles of H2O produced, we use the mole ratio between Al(OH)3 and H2O. From the balanced equation, we can see that the ratio is 1 mole of H2O to 1 mole of Al(OH)3.
6. To calculate the moles of H2O produced, we multiply the moles of Al(OH)3 by its mole ratio:
moles of H2O = moles of Al(OH)3
7. Finally, to find the mass of H2O produced, we multiply the moles of H2O by its molar mass:
mass of H2O = moles of H2O * molar mass of H2O
It's important to note that the molar masses of HCl and H2O need to be determined using the periodic table and must have at least as many significant figures as the given data.