Waiting for answer This question has not been answered yet. You can hire a professional tutor to get the answer.

QUESTION

# Diphosphorus pentoxide reacts with water to produce phosphoric acid (H_3PO_4). How do you write the balanced equation for this reaction?

"P"_4"O"_text(10(s]) + 6"H"_2"O"_text((l]) -> 4"H"_3"PO"_text(4(aq])

The interesting thing about diphosphorus pentoxide, "P"_2"O"_5, is that it usually exists as a dimer.

This implies that "P"_2"O"_5 is actually the compound's and that you should use "P"_4"O"_10 as its molecular formula.

Now, diphosphorus pentoxide reacts violently with water to form phosphoric acid, "H"_3"PO"_4. The reaction is highly exothermic and leads to the formation of toxic fumes.

The unbalanced chemical equation for this reaction looks like this

"P"_4"O"_text(10(s]) + "H"_2"O"_text((l]) -> "H"_3"PO"_text(4(aq])

To balance this equation, start by multiplying the phosphoric acid by 4 to get equal numbers of atoms of phosphorus on both sides of the equation

"P"_4"O"_text(10(s]) + "H"_2"O"_text((l]) -> 4"H"_3"PO"_text(4(aq])

Notice that you have 2 atoms of hydrogen on the reactants' side and 12 on the products' side. Multiply the water molecule by 6 to balance the hydrogen atoms out.

Incidentally, this will also balance out the atoms of oxygen, since you'd now have 16 on the reactants' side and 16 on the products' side.

The balanced chemical equation for this reaction will thus be

"P"_4"O"_text(10(s]) + 6"H"_2"O"_text((l]) -> 4"H"_3"PO"_text(4(aq])

It's worth mentioning that diphosphorus pentoxide is a very powerful dehydrating agent.

SIDE NOTE You'll sometimes see this reaction written using the empirical formula of diphosphorus pentoxide, "P"_2"O"_5. In that case, the balanced chemical equation will be

"P"_2"O"_text(5(s]) + 3"H"_2"O"_text((l]) -> 2"H"_3"PO"_text(4(aq])