How many moles of H3PO4 are produced when 142.0 g P4O10 reacts completely to form H3PO4?
See example below.
Oh, moles and moles! I love a good chemistry joke! Ok, so let's calculate this. We'll start by finding the molar mass of P4O10. The atomic mass of phosphorus is around 31 grams per mole, and the atomic mass of oxygen is around 16 grams per mole. P4O10 has four phosphorus atoms and ten oxygen atoms, so the molar mass is (4 * 31) + (10 * 16) = 284 grams per mole. Now, we can use stoichiometry to find the number of moles of H3PO4 produced. From the balanced equation, we know that 1 mole of P4O10 reacts to form 6 moles of H3PO4. So, using the molar mass of P4O10, we have (142.0 g / 284 g/mol) * 6 mol H3PO4/mol P4O10 = 3 moles of H3PO4. Voila! Three moles of H3PO4 are produced. Now that's a lot of moles, not the furry kind though!
We can start by writing the balanced equation for the reaction of P4O10 with H3PO4:
P4O10 + 6H2O -> 4H3PO4
The molar mass of P4O10 is 283.89 g/mol, and the molar mass of H3PO4 is 97.99 g/mol.
Step 1: Calculate the number of moles of P4O10.
To do this, we can use the formula:
moles = mass / molar mass
moles of P4O10 = 142.0 g / 283.89 g/mol = 0.5 mol
Step 2: Determine the mole ratio between P4O10 and H3PO4.
From the balanced equation, we can see that 1 mol of P4O10 reacts to produce 4 mol of H3PO4.
Step 3: Calculate the number of moles of H3PO4 produced.
To do this, we can use the mole ratio:
moles of H3PO4 = moles of P4O10 x (moles of H3PO4 / moles of P4O10)
moles of H3PO4 = 0.5 mol x (4 mol H3PO4 / 1 mol P4O10) = 2 mol
Therefore, when 142.0 g of P4O10 reacts completely, 2 moles of H3PO4 are produced.
To determine the number of moles of H3PO4 produced when 142.0 g P4O10 reacts completely, you need to follow these steps:
Step 1: Write the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction is:
P4O10 + 6H2O -> 4H3PO4
Step 2: Calculate the molar mass of P4O10.
The molar mass of P4O10 can be calculated by adding up the atomic masses of each element:
Molar mass of P4O10 = (4 * atomic mass of P) + (10 * atomic mass of O)
= (4 * 30.97 g/mol) + (10 * 16.00 g/mol)
= 123.88 g/mol + 160.00 g/mol
= 283.88 g/mol
Step 3: Convert the given mass of P4O10 to moles.
To convert grams to moles, divide the given mass by the molar mass:
Number of moles of P4O10 = mass of P4O10 / molar mass of P4O10
= 142.0 g / 283.88 g/mol
≈ 0.500 mol (rounded to three significant figures)
Step 4: Use stoichiometry to find the moles of H3PO4 produced.
From the balanced chemical equation, we see that one mole of P4O10 reacts to produce four moles of H3PO4. Therefore, the number of moles of H3PO4 produced is:
Number of moles of H3PO4 = 4 * number of moles of P4O10
= 4 * 0.500 mol
= 2.000 mol
Therefore, 2.000 moles of H3PO4 are produced when 142.0 g P4O10 reacts completely.