What mass of phosphoric acid will be produced from the reaction of 10.00g of P4O10 with excess water?
P4O10 + 6H2O ==> 4H3PO4
Convert 10.00 g P4O10 to moles. # moles = grams/molar mass.
Using the coefficients in the balanced equation, convert moles P4O10 to moles H3PO4.
Convert moles H3PO4 to grams.
grams = moles x molar mass.
The balanced chemical equation for the reaction is:
P4O10 + 6H2O -> 4H3PO4
From the balanced equation, we can see that 1 mole of P4O10 will produce 4 moles of H3PO4.
1 mole of P4O10 has a molar mass of 283.88 g/mol.
To find the number of moles of P4O10 in 10.00g, we divide the mass by the molar mass:
moles of P4O10 = 10.00g / 283.88 g/mol = 0.0352 mol
Since the ratio of P4O10 to H3PO4 is 1:4, the number of moles of H3PO4 produced will be four times the number of moles of P4O10:
moles of H3PO4 = 4 * 0.0352 mol = 0.1408 mol
The molar mass of H3PO4 is 97.99 g/mol.
To find the mass of H3PO4 produced, we multiply the number of moles by the molar mass:
mass of H3PO4 = 0.1408 mol * 97.99 g/mol = 13.79 g
Therefore, the mass of phosphoric acid produced from the reaction of 10.00g of P4O10 with excess water is 13.79 g.
To calculate the mass of phosphoric acid produced from the reaction of P4O10 with water, we first need to write a balanced chemical equation for the reaction.
The balanced equation for the reaction between P4O10 and water is:
P4O10 + 6 H2O -> 4 H3PO4
From the balanced equation, we can see that one mole of P4O10 reacts with six moles of water to produce four moles of phosphoric acid (H3PO4).
To calculate the number of moles of P4O10, we need to convert the given mass of P4O10 into moles. The molar mass of P4O10 can be calculated by adding the atomic masses of the individual elements:
P4O10: (4 * atomic mass of P) + (10 * atomic mass of O)
P: 4 * 30.97 g/mol = 123.88 g/mol
O: 10 * 16.00 g/mol = 160.00 g/mol
Molar mass of P4O10: 123.88 g/mol + 160.00 g/mol = 283.88 g/mol
Now, we can calculate the number of moles of P4O10:
moles of P4O10 = mass of P4O10 / molar mass of P4O10
moles of P4O10 = 10.00 g / 283.88 g/mol = 0.0352 mol
Since the reaction is balanced in a 1:4 ratio between P4O10 and H3PO4, we can determine the number of moles of H3PO4 produced:
moles of H3PO4 = 4 * moles of P4O10
moles of H3PO4 = 4 * 0.0352 mol = 0.1408 mol
Finally, we can calculate the mass of H3PO4 produced by multiplying the number of moles by its molar mass:
mass of H3PO4 = moles of H3PO4 * molar mass of H3PO4
mass of H3PO4 = 0.1408 mol * (1 * 1.01 g/mol + 4 * 16.00 g/mol) = 0.1408 mol * 98.09 g/mol = 13.83 g
Therefore, 13.83 grams of phosphoric acid (H3PO4) will be produced from the reaction of 10.00 grams of P4O10 with excess water.