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Aleksandr [31]
3 years ago
15

When 0.422g of phosphorus is burned, 0.967g of a white oxide is obtained.

Chemistry
2 answers:
slava [35]3 years ago
7 0

Answer :

(a) The empirical formula of a compound is, P_2O_5

(b) The balanced chemical equation will be:

P_4+5O_2\rightarrow 2P_2O_5

Solution :  Given,

Mass of phosphorus = 0.422 g

Mass of white oxide = 0.967 g

Molar mass of phosphorus = 31 g/mole

Molar mass of oxygen = 16 g/mole

First we have to calculate the mass of oxygen.

Mass of oxygen = Mass of white oxide - Mass of phosphorus

Mass of oxygen = 0.967 - 0.422

Mass of oxygen = 0.545 g

Now convert given masses into moles.

Moles of P = \frac{\text{ given mass of P}}{\text{ molar mass of P}}= \frac{0.422g}{31g/mole}=0.0136moles

Moles of O = \frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{0.545g}{16g/mole}=0.0341moles

For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For P = \frac{0.0136}{0.0136}=1

For O = \frac{0.0341}{0.0136}=2.5

The ratio of P : O = 1 : 2.5

To make this ratio in a whole number we multiple ratio by 2, we get:

The ratio of P : O = 2 : 5

The mole ratio of the element is represented by subscripts in empirical formula.

The Empirical formula = P_2O_5

The balanced chemical equation will be:

P_4+5O_2\rightarrow 2P_2O_5

nata0808 [166]3 years ago
5 0
Moles = mass / molar mass 

<span>moles P = 0.422 g / 30.97 g/mol = 0.01363 mol </span>
<span>moles O = (0.967 g - 0.422g) / 16.00 g/mol = 0.03406 moles </span>

<span>So ratio moles P : moles O </span>
<span>= 0.01363 mol : 0.03406 mol </span>

<span>Divide each number in the ratio by the smallest number </span>

<span>(0.01363 / 0.01363) : (0.03406 / 0.01363) </span>
<span>= 1 : 2.5 </span>

<span>The empirical formula needs to be the smallest whole number ratio of atoms in the molecules. Since you have a non-whole number, multiply the ratio by the smallest number needed to make both number whole numbers. In this case x 2 </span>

<span>2 x (1 : 2.5) </span>
<span>= 2 : 5 </span>
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