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Chapter 3: Problem 43

Phosphorus reacts with oxygen to produce different kinds of oxides. One of these oxides is formed when \(1.347 \mathrm{~g}\) of phosphorus reacts with \(1.744 \mathrm{~g}\) of oxygen. What is the simplest formula of this oxide? Name the oxide.

Short Answer

Expert verified
Answer: The simplest formula of the oxide is P2O5 and its name is diphosphorus pentoxide.

Step by step solution

01

Calculate moles of phosphorus and oxygen

To find the moles of each element, we need to use their respective molar masses. The molar mass of phosphorus (P) is 30.97 g/mol and the molar mass of oxygen (O) is 16.00 g/mol. We'll use the equation: moles = mass (g) / molar mass (g/mol) For phosphorus: moles of P = 1.347 g / 30.97 g/mol = 0.0435 mol For oxygen: moles of O = 1.744 g / 16.00 g/mol = 0.109 mol
02

Divide both quantities by the smallest number of moles

Now, we need to find the molar ratio between phosphorus and oxygen in the oxide. We'll do this by dividing both quantities by the smallest number of moles: Minimum moles = 0.0435 mol Phosphorus molar ratio = 0.0435 mol / 0.0435 mol = 1 Oxygen molar ratio = 0.109 mol / 0.0435 mol ≈ 2.5
03

Simplify and find the empirical formula

We have a ratio of approximately 1:2.5 for phosphorus and oxygen, which we need to simplify. Since 2.5 is close to 2, we'll multiply the ratio by 2 to get whole numbers: Phosphorus ratio * 2 = 1 * 2 = 2 Oxygen ratio * 2 = 2.5 * 2 = 5 Now we see that there are 2 phosphorus atoms and 5 oxygen atoms in the simplest formula. So, the empirical formula is P2O5.
04

Name the oxide

Based on the empirical formula P2O5, we can name the oxide as diphosphorus pentoxide. This is the simplest formula and name of the oxide produced when 1.347 g of phosphorus reacts with 1.744 g of oxygen.

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