How many liters of oxygen a@STP will produce 195 grams of diphosphorus pentoxide when reacted with sufficient phosphorus?- exact question. Could someone plz help I am confused and if you could help me put it in dimensional analysis.

4P + 5O2 --> 2P2O5

Convert g P205 to mol.
195g P2O5 x (1 mol P2O5/molar mass P2O5) = ?

Convert mols P2O5 to mols O2.
?mols P2O5 x (5 mol O2/2 mol P2O5) = ?

volume O2 produced = mols O2 x (22.4L/mol) = ?

To solve this problem using dimensional analysis, we need to go through the following steps:

Step 1: Understand the given information
Given: 195 grams of diphosphorus pentoxide (P2O5) and sufficient phosphorus react.
We need to find the volume of oxygen produced at STP.

Step 2: Write down the balanced chemical equation
The balanced equation for the reaction between phosphorus and diphosphorus pentoxide is:
4P + 5O2 -> 2P2O5

From the equation, we can see that four moles of phosphorus react with five moles of oxygen to produce two moles of diphosphorus pentoxide.

Step 3: Convert grams of P2O5 to moles
To convert the given grams of diphosphorus pentoxide (P2O5) to moles, we need to know the molar mass of P2O5. The molar mass can be calculated as follows:
Molar mass of P2O5 = (2 * atomic mass of phosphorus) + (5 * atomic mass of oxygen)
= (2 * 31.0 g/mol) + (5 * 16.0 g/mol)
= 62.0 g/mol + 80.0 g/mol
= 142.0 g/mol

Now, we can calculate the number of moles of P2O5 using the given mass:
Moles of P2O5 = Given mass / Molar mass
= 195 g / 142.0 g/mol
= 1.373 moles

Step 4: Determine the moles of oxygen required
From the balanced chemical equation, we can see that 5 moles of oxygen are required to react with 2 moles of P2O5. So, we can set up a proportion:

(5 moles O2) / (2 moles P2O5) = (x moles O2) / (1.373 moles P2O5)

We can solve this proportion to find the moles of oxygen required.

Step 5: Convert moles of oxygen to volume at STP
At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 liters of volume. So, we can use this conversion factor to convert the moles of oxygen into liters.

Step 6: Calculate the final answer
Multiply the moles of oxygen by the conversion factor (22.4 L/mol) to obtain the volume of oxygen at STP.

It's important to note that the problem statement does not specify how much phosphorus is reacted, so this method assumes that it is in excess and is not limiting the reaction.

I hope this explanation helps you understand how to use dimensional analysis to solve this type of problem.