A mass of 11.6g of phosphoric acid was produced from the reaction of 10g of P4O10 with 12g of water. What was the percent yield for this reaction?
P4O10+6H2O>> 4H3PO4
The percent yield: massobtained/massreacted= 11.6/(10+12) change that to percent.
To find the percent yield of a reaction, we need to compare the actual yield to the theoretical yield and calculate the ratio. The formula for percent yield is:
Percent yield = (actual yield / theoretical yield) x 100%
First, we need to determine the moles of P4O10 and H2O used:
Molar mass of P4O10 = 4 (molar mass of P) + 10 (molar mass of O)
= 4 (30.97 g/mol) + 10 (16.00 g/mol)
= 123.88 g/mol
Moles of P4O10 = mass / molar mass = 10 g / 123.88 g/mol
Molar mass of H2O = (2 x molar mass of H) + molar mass of O
= (2 x 1.01 g/mol) + 16.00 g/mol
= 18.02 g/mol
Moles of H2O = mass / molar mass = 12 g / 18.02 g/mol
Next, we need to calculate the limiting reactant by comparing the ratio of moles of P4O10 to H2O. The reactant that produces the least number of moles of products is the limiting reactant. The balanced equation for the reaction is:
P4O10 + 6H2O → 4H3PO4
According to the balanced equation, 1 mole of P4O10 reacts to produce 4 moles of H3PO4.
Moles of H3PO4 produced from P4O10 = moles of P4O10 x (4 moles H3PO4 / 1 mole P4O10)
Moles of H3PO4 = (10 g / 123.88 g/mol) x (4 mol H3PO4 / 1 mol P4O10)
Finally, calculate the theoretical yield of phosphoric acid:
Theoretical yield = moles of H3PO4 x molar mass of H3PO4
Now, calculate the actual yield of phosphoric acid based on the given mass:
Actual yield = 11.6 g
Now we can calculate the percent yield:
Percent yield = (actual yield / theoretical yield) x 100%
= (11.6 g / theoretical yield) x 100%
Please provide the molar mass of phosphoric acid (H3PO4) so we can calculate the theoretical yield and determine the percent yield for this reaction.
To calculate the percent yield for a reaction, you need to compare the actual yield with the theoretical yield.
First, let's find the molar mass of P4O10 and H3PO4 (phosphoric acid) to determine the chemical equation's stoichiometry.
The molar mass of P4O10 = 4 atoms of phosphorus (4 * 31.0 g/mol) + 10 atoms of oxygen (10 * 16.0 g/mol) = 284.0 g/mol.
The balanced chemical equation for the reaction between P4O10 and H2O is:
P4O10 + 6H2O ➜ 4H3PO4
From the equation, we can observe that 1 mole of P4O10 reacts with 6 moles of H2O to produce 4 moles of H3PO4.
Now, let's calculate the theoretical yield of phosphoric acid (H3PO4).
Step 1: Convert the given mass of P4O10 (10g) to moles using the molar mass:
10g P4O10 * (1 mol P4O10 / 284.0 g P4O10) = 0.0352 mol P4O10
Step 2: Determine the number of moles of H3PO4 produced, using the stoichiometry from the balanced equation:
0.0352 mol P4O10 * (4 mol H3PO4 / 1 mol P4O10) = 0.1408 mol H3PO4
Step 3: Convert moles of H3PO4 to grams of H3PO4 using the molar mass:
0.1408 mol H3PO4 * (98.0 g H3PO4 / 1 mol H3PO4) = 13.8 g H3PO4
So, the theoretical yield of phosphoric acid is 13.8 g.
Now, let's find the actual yield. The given mass of phosphoric acid produced is 11.6 g.
To calculate the percent yield, use the formula:
Percent Yield = (Actual Yield / Theoretical Yield) * 100
Plugging in the values:
Percent Yield = (11.6 g / 13.8 g) * 100 = 83.9%
Therefore, the percent yield for this reaction is 83.9%.