# How you solve P4(s)+5O2(g)------>P4O10(g) .if 2.50 grams of phosphorus is ignited in a flask how many grams of P4O10 are formed ?

## 1. mols P = grams/molar mass

2. Convert mols P to mols P4O10 using the coefficients in the balanced equation.
3. Convert mols P4O10 to g. g = mols x molar mass.

## To determine the grams of P4O10 formed, we need to use stoichiometry, which involves the use of balanced chemical equations. The balanced equation for the reaction is:

P4(s) + 5O2(g) → P4O10(g)

The molar ratio between P4 and P4O10 is 1:1, meaning for every 1 mole of P4, we will have 1 mole of P4O10.

To solve the problem, follow these steps:

Step 1: Convert grams of P4 to moles.
We will use the molar mass of P4 to convert grams to moles. The molar mass of phosphorus (P) is 31 grams/mole.

Using the formula: Moles = Mass / Molar mass

Moles of P4 = 2.50 g / (31 g/mol) = 0.0806 mol

Step 2: Use the stoichiometric coefficients to determine the moles of P4O10.
Since the molar ratio between P4 and P4O10 is 1:1, the moles of P4O10 will be equal to the moles of P4.

Moles of P4O10 = 0.0806 mol

Step 3: Convert moles of P4O10 to grams.
To convert moles of P4O10 to grams, we will use the molar mass of P4O10. The molar mass of P4O10 is 283.9 g/mol.

Using the formula: Mass = Moles × Molar mass

Mass of P4O10 = 0.0806 mol × (283.9 g/mol) = 22.9 g

Therefore, 2.50 grams of phosphorus will produce 22.9 grams of P4O10.

## To solve this problem, we need to use stoichiometry, which is based on the balanced chemical equation. The balanced chemical equation for the reaction given is:

P4(s) + 5O2(g) → P4O10(g)

From this equation, we can see that 1 mole of P4 reacts to form 1 mole of P4O10. This means the molar ratio between P4 and P4O10 is 1:1.

First, let's calculate the number of moles of phosphorus (P4) using its molar mass. The molar mass of phosphorus is 31.0 g/mol.
Number of moles of P4 = mass of P4 / molar mass of P4
= 2.50 g / 31.0 g/mol
= 0.0806 mol (rounded to four decimal places)

Since the molar ratio between P4 and P4O10 is 1:1, the number of moles of P4O10 formed will also be 0.0806 mol.

Now, let's calculate the mass of P4O10 using its molar mass. The molar mass of P4O10 is calculated by summing up the molar masses of the elements in P4O10.
Molar mass of P4O10 = (molar mass of P4) + 10 × (molar mass of O)
= 123.9 g/mol

Mass of P4O10 = number of moles of P4O10 × molar mass of P4O10
= 0.0806 mol × 123.9 g/mol
= 10.0 g (rounded to one decimal place)

Therefore, if 2.50 grams of P4 is ignited, approximately 10.0 grams of P4O10 will be formed.