What mass of PCl3 forms in the reaction of 70.6 g P4 with 268 g Cl2 ?
P4 + 6Cl2 → 4PCl3
hom many moles of P4 do you have.
how many moles of CL2 do you have.
figure those.
Now, if you have less than six Cl2 moles for the moles of P4, then CL2 is the limiting reagent. The product will equal 4/6 of the moles of CL2 you have.
If you have more than six moles of Cl2 for the moles of P4, then P4 is the limiting reagent, and you will get four times the P4 moles , as the product PCl3
To find the mass of PCl3 formed in the reaction, we need to use stoichiometry to determine the molar ratio between P4 and PCl3. Here's how to do it step by step:
Step 1: Calculate the number of moles of P4 and Cl2.
First, calculate the number of moles for P4:
Number of moles of P4 = Mass of P4 / Molar mass of P4.
The molar mass of P4 can be calculated using the periodic table. The atomic mass of phosphorus (P) is approximately 31.0 g/mol, so the molar mass of P4 is:
Molar mass of P4 = 4 * Atomic mass of P = 4 * 31.0 g/mol = 124.0 g/mol.
Now, calculate the number of moles of P4:
Number of moles of P4 = 70.6 g P4 / 124.0 g/mol = 0.569 moles.
Similarly, calculate the number of moles of Cl2 using its molar mass. The atomic mass of chlorine (Cl) is approximately 35.5 g/mol, so the molar mass of Cl2 is:
Molar mass of Cl2 = 2 * Atomic mass of Cl = 2 * 35.5 g/mol = 71.0 g/mol.
Number of moles of Cl2 = 268 g Cl2 / 71.0 g/mol = 3.77 moles.
Step 2: Determine the limiting reactant.
Compare the number of moles of each reactant to find the limiting reactant. The limiting reactant is the one that is completely consumed in the reaction and determines the maximum amount of product formed.
Using the balanced equation, we can see that the stoichiometric ratio between P4 and PCl3 is 1:4 (1 P4 produces 4 PCl3).
Since we have 0.569 moles of P4 and the stoichiometric ratio is 1:4, the expected number of moles of PCl3 would be:
Expected number of moles of PCl3 = 0.569 moles P4 * 4 moles PCl3 / 1 mole P4 = 2.276 moles.
Similarly, for Cl2, the stoichiometric ratio is 6:4 (6 Cl2 produces 4 PCl3), so the expected number of moles of PCl3 would be:
Expected number of moles of PCl3 = 3.77 moles Cl2 * 4 moles PCl3 / 6 moles Cl2 = 2.513 moles.
Comparing the calculated number of moles of PCl3, we see that 2.276 moles (from P4) is smaller than 2.513 moles (from Cl2). Therefore, P4 is the limiting reactant.
Step 3: Calculate the mass of PCl3 formed.
Now that we know the limiting reactant is P4 and we have the stoichiometric ratio of 1:4 between P4 and PCl3, we can calculate the number of moles of PCl3 produced.
Number of moles of PCl3 = Number of moles of limiting reactant (P4) * Stoichiometric ratio = 0.569 moles * 4 moles PCl3 / 1 mole P4 = 2.276 moles.
Finally, calculate the mass of PCl3 formed using its molar mass:
Mass of PCl3 = Number of moles of PCl3 * Molar mass of PCl3.
The molar mass of PCl3 can be calculated using the atomic masses of phosphorus (P) and chlorine (Cl):
Molar mass of PCl3 = Atomic mass of P + 3 * Atomic mass of Cl = 31.0 g/mol + 3 * 35.5 g/mol = 137.5 g/mol.
Mass of PCl3 = 2.276 moles PCl3 * 137.5 g/mol = 312.17 g.
Therefore, the mass of PCl3 formed in the reaction is approximately 312.17 g.
To find the mass of PCl3 formed, we first need to determine which reactant is limiting. This can be done by comparing the amount of moles of each reactant.
1. Calculate the number of moles of P4:
Molar mass of P4 = 4 * atomic mass of P = 4 * 31.0 g/mol = 124.0 g/mol
Number of moles of P4 = mass of P4 / molar mass of P4
= 70.6 g / 124.0 g/mol
≈ 0.569 moles
2. Calculate the number of moles of Cl2:
Molar mass of Cl2 = 2 * atomic mass of Cl = 2 * 35.5 g/mol = 71.0 g/mol
Number of moles of Cl2 = mass of Cl2 / molar mass of Cl2
= 268 g / 71.0 g/mol
≈ 3.77 moles
3. Determine the stoichiometric ratio:
From the balanced equation: P4 + 6Cl2 → 4PCl3
We can see that it requires 1 mole of P4 to react with 6 moles of Cl2, producing 4 moles of PCl3.
4. Calculate the number of moles of PCl3 that can be formed:
Since P4 is the limiting reactant, we need to calculate how many moles of PCl3 can be formed from the moles of P4.
Number of moles of PCl3 = moles of P4 * stoichiometric ratio
= 0.569 moles * (4 moles PCl3 / 1 mole P4)
= 2.276 moles
5. Calculate the mass of PCl3 formed:
Molar mass of PCl3 = 1 * atomic mass of P + 3 * atomic mass of Cl = 1 * 31.0 g/mol + 3 * 35.5 g/mol = 137.5 g/mol
Mass of PCl3 = number of moles of PCl3 * molar mass of PCl3
= 2.276 moles * 137.5 g/mol
≈ 312.1 g
Therefore, approximately 312.1 g of PCl3 will be formed in the reaction.