How many grams of air are required to complete the combustion of 120 g of phosphorous to diphosphorous pentoxide, assuming the air to be 23% oxygen by mass?

Explanation:

522 g

Explanation:

Your starting point here will be the balanced chemical equation for this combustion reaction

4

P

(s]

+

5

O

2(g]

→

2

P

2

O

5(s]

Notice that you have a

4

:

5

mole ratio between phosphorus and oxygen. This means that, regardless of how many moles of phosphorus you have, the reaction will always need

5

4

time more moles of oxygen gas.

Use phosphorus' molar mass to determine how many moles you have in that

93.0-g

sample

93.0

g

⋅

1mole P

30.974

g

=

3.0025 moles P

Use the aforementioned mole ratio to determine how many moles of oxygen you would need for many moles of phosphorus to completely take part in the reaction

3.0025

moles P

⋅

5

moles O

2

4

moles P

=

3.753 moles O

2

the food using pesticides in the future will harm you by giving you diseases like cancer or something since they have things that we should not eat in it like chemicals or pesticides. that is why organic food is more expensive because they take the time to make it right and healthy for you to eat.

explanation: