Question

Simplest formula of compound containing 21.9 percent of magnesium, 27.8percent of phosphorus, 50.3percent of oxygen

Answer 1

simplest formula is nothing but emperical formula. ans may be MgPO3
please tell is it correct

Answer 2

The empirical formula for the given compound is $Mg_2P_2O_7$

Explanation:

We are given:

Percentage of Mg = 21.9 %

Percentage of P = 27.8 %

Percentage of O = 50.3 %

Let the mass of compound be 100 g. So, percentages given are taken as mass.

Mass of Mg = 21.9 g

Mass of P = 27.8 g

Mass of O = 50.3 g

To formulate the empirical formula, we need to follow some steps:

• Step 1: Converting the given masses into moles.

Moles of Magnesium =$\frac{\text{Given mass of Magnesium}}{\text{Molar mass of Magnesium}}=\frac{21.9g}{24g/mole}=0.9125moles$

Moles of Phosphorus = $\frac{\text{Given mass of Phosphorus}}{\text{Molar mass of Phosphorus}}=\frac{27.8g}{31g/mole}=0.897moles$

Moles of Oxygen = $\frac{\text{Given mass of Oxygen}}{\text{Molar mass of Oxygen}}=\frac{50.3g}{16g/mole}=3.144moles$

• Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.897 moles.

For Magnesium = $\frac{0.9125}{0.897}=1.012\approx 1$

For Phosphorus = $\frac{0.897}{0.897}=1$

For Oxygen = $\frac{3.144}{0.897}=3.5$

To make the subscript a whole number, we multiply the mole ratios by '2'

Mole ratio of magnesium = $(1\times 2)=2$

Mole ratio of phosphorus = $(1\times 2)=2$

Mole ratio of oxygen = $(3.5\times 2)=7$

• Step 3: Taking the mole ratio as their subscripts.

The ratio of Mg : P : O = 2 : 2 : 7

Learn more about empirical formula:

https://brainly.in/question/11318410

https://brainly.com/question/13179835

#learnwithbrainly