Question

In part a, you found the amount of product (3.00 mol p2o5 ) formed from the given amount of phosphorus and excess oxygen. in part b, you found the amount of product (2.60 mol p2o5 ) formed from the given amount of oxygen and excess phosphorus.now, determine how many moles of p2o5 are produced from the given amounts of phosphorus and oxygen.express your answer to three significant figures and include the appropriate units.

Answer 1

Answer is: 2,6 moles of P₂O₅ are produced from the given amounts of phosphorus and oxygen.
Chemical reaction: P₄ + 5O₂ → 2P₂O₅.
m(P₄) = 186 g.
n(P₄) = m(P₄) ÷ M(P₄).
n(P₄) = 186 g ÷ 123,9 g/mol.
n(P₄) = 1,5 mol.
m(O₂) = 208 g.
n(O₂) = 208 g ÷ 32 g/mol.
n(O₂) = 6,5 mol; limiting reactant.
From chemical reaction: n(O₂) : n(P₂O₅) = 5 : 2.
n(P₂O₅) = 2 · 6,5 mol ÷ 5.
n(P₂O₅) = 2,6 mol.

Answer 2

The correct answer is 2.60 moles.

Step-by-step explanation:

The balanced equation is:

4P + 5O₂ ⇒ 2P₂O₅

The number of moles of O₂, n = mass/molar mass

208 g / 32 g/mol = 6.5 mol

From the balanced equation,

5 moles of O₂ reacts with 2 moles of P₂O₅

So, 6.5 moles of O₂ reacts with M moles of P₂O₅

M = 6.5 × 2/5

= 2.6 moles

Therefore, the required moles of P₂O₅ are 2.60 moles.