PbO2 + 2H2 = Pb + 2H2O
If 478g of lead doixide is heated, what is:
a. the number of moles of lead dioxide used?
b. the number of moles of lead produced?
c. the mass of lead produced?
I am stuck.... please help!!
I DONT KNOW PLS HELP
To solve this problem, we will use the concept of stoichiometry, which involves calculating the relationship between the amounts of reactants and products in a chemical reaction.
First, let's write the balanced equation for the reaction:
PbO2 + 2H2 -> Pb + 2H2O
a. To find the number of moles of lead dioxide used, we need to convert the given mass into moles. We can do this by using the molar mass of PbO2.
The molar mass of PbO2 can be calculated by adding the atomic masses of its components:
Pb (lead) = 207.2 g/mol
O (oxygen) = 16.0 g/mol (there are two oxygen atoms in PbO2)
So, the molar mass of PbO2 = 207.2 g/mol + (2 * 16.0 g/mol) = 239.2 g/mol.
Now, we can find the number of moles of PbO2:
Number of moles = Mass of PbO2 / Molar mass of PbO2
Number of moles = 478 g / 239.2 g/mol
b. To find the number of moles of lead produced, we use the balanced equation. From the equation, we can see that the stoichiometric ratio between PbO2 and Pb is 1:1. So, the number of moles of Pb produced will be equal to the number of moles of PbO2 used.
c. To calculate the mass of lead produced, we can use the molar mass of Pb:
The molar mass of Pb is 207.2 g/mol.
Mass of Pb produced = Number of moles of Pb * Molar mass of Pb
I hope this helps! Let me know if you have any further questions.
Very good
a. mols PbO2 = grams/molar mass = ?
b. 1 mol PbO2 produces 1 mol Pb; therefore, mols Pb = mols PbO2.
c. grams Pb = mols Pb x atomic mass Pb.
Remember this. This will work all of your stoichiometry problems. Step #1 is to write the balanced equation but you already had that.