Tetraphosphorus trisulphide (P4S3) is used in the match heads of some matches. It is produced in the reaction 8P4+3S8 --> 8P4S3. Determine which of the following statements are incorrect, and rewrite the incorrect statements to make them correct.

a. 4 mol P4 reacts with 1.5 mol S8 to form 4 mol P4S3
b. sulfur is the limiting reactant when 4 mol P4 and 4 mol S8 react.
c. 6 mol P4 reacts with 6 mol S8 forming 1320 g P4S3.

I don't get how to do this! If I just get an idea of how to set it up then I can figure it out! And for the first one I think it is incorrect, but I'm not sure...? Thanks!!

a is correct.

4 moles P4/8 moles P4 = 1/2 as much.
1.5 is 1/2 of 3 for S
4 is 1/2 8 for P4S3.
All of the ratios stayed the same; therefore, you've simply cut the reaction in 1/2.

b. Do this twice to make sure you are right. Use the coefficients in the balanced equation.
(1) compare P to S
(2) compare S to P.
(1)4 mol P4 should take 1.5 mol S8. Do you have 1.5 mols S8? yes, you have 4 moles; therefore, you have more than enough S8 to react so P MUST THE THE LIMITING REAGENT.
(2) We think we know the answer but we do this to make sure we are right.
4 mol S8 *(8 moles P4/3 moles S8) = 10.7 moles P4 needed to react with 4 mol S8. Do we have 10.7 moles P4? No, we have only 4; therefore, P must be the limiting reagent.
c. This is a limiting reagent problem. Determine which is the limiting reagent, use that and the coefficients to convert the amount of the limiting reagent to moles of the product, then convert mols product to grams of product and see if that equals 1320 g.

1

a. 4 mol P4 reacts with 1.5 mol S8 to form 6 mol P4S3. (Correction: The balanced equation shows that the ratio between P4 and S8 is 8:3, so you would need 4 mol of P4 to react with (3/8) * 4 mol of S8, which equals 1.5 mol of S8. The product formed in this case would be 6 mol of P4S3.)

b. Sulfur is the limiting reactant when 8 mol P4 and 3 mol S8 react. (Correction: According to the balanced equation, the ratio between P4 and S8 is 8:3. Therefore, you would need (8/8) * 3 mol of S8, which equals 3 mol of S8, to react with 8 mol of P4. Since you have 3 mol of S8, this means that sulfur is not the limiting reactant; you have enough sulfur to react with all the phosphorus.)

c. 6 mol P4 reacts with 2.25 mol S8 forming 396 g P4S3. (Correction: To determine the mass of P4S3, you need to know the molar mass of P4S3. Based on its formula, the molar mass of P4S3 is approximately 220 g/mol. Therefore, you can calculate the mass of P4S3 by multiplying the number of moles (6 mol) by the molar mass (220 g/mol). This gives you a mass of 1320 g P4S3, which means the statement is correct as it is.)

To determine which statements are incorrect, we need to calculate the correct stoichiometric ratios and then compare them to the given statements.

Let's start by balancing the chemical equation:

8P4 + 3S8 → 8P4S3

The balanced equation tells us that 8 moles of P4 react with 3 moles of S8 to form 8 moles of P4S3.

Now, let's analyze each statement:

a. 4 mol P4 reacts with 1.5 mol S8 to form 4 mol P4S3.

To determine if this statement is correct, we need to calculate the stoichiometric ratio using the balanced equation. From the balanced equation, we observe that the ratio of P4 to S8 is 8:3. Therefore, for 4 moles of P4, the corresponding amount of S8 needed would be:

(4 moles P4) x (3 moles S8 / 8 moles P4) = 1.5 moles S8

This means that statement a is correct. No correction is required.

b. Sulfur is the limiting reactant when 4 mol P4 and 4 mol S8 react.

To determine the limiting reactant, we need to calculate the moles of each reactant and compare them based on the stoichiometry of the balanced equation. From the balanced equation, we know that the stoichiometric ratio of P4 to S8 is 8:3.

For 4 moles of P4, the corresponding amount of S8 needed would be:

(4 moles P4) x (3 moles S8 / 8 moles P4) = 1.5 moles S8

Comparing this calculation to the given statement, we can see that the amount of S8 required is less than the given 4 mol S8. Therefore, sulfur is not the limiting reactant in this case. The correct statement would be:

"Phosphorus is the limiting reactant when 4 mol P4 and 4 mol S8 react."

c. 6 mol P4 reacts with 6 mol S8 forming 1320 g P4S3.

To determine if this statement is correct, we need to calculate the molar mass of P4S3 and convert the given moles into grams.

The molar mass of P4S3 is:

(4P x Atomic mass of P) + (3S x Atomic mass of S)
= (4 x 31 g/mol) + (3 x 32 g/mol)
= 124 g/mol + 96 g/mol
= 220 g/mol

Now, let's calculate the mass of P4S3 formed when 6 moles of P4 react:

(6 moles P4S3) x (220 g P4S3 / 1 mol P4S3) = 1320 g P4S3

This means that statement c is correct. No correction is required.

In summary, the incorrect statement is:

b. Sulfur is the limiting reactant when 4 mol P4 and 4 mol S8 react.

The corrected statement would be:

"Phosphorus is the limiting reactant when 4 mol P4 and 4 mol S8 react."

___si___+s8>si2s4

no