Question

The simplest formula of a compound that containing 81.8 carbon and 18.2 hydrogen

Answer 1

THE SIMPLEST FORMULA OF THE COMPOUND IS CH4 THAT MEANS MEATHEN

Answer 2

The empirical formula for the given compound is $CH_2$

Explanation:

We are given:

Percentage of C = 81.8 %

Percentage of H = 18.2 %

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

Mass of C = 81.8 g

Mass of H = 18.2 g

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

• Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{81.8g}{12g/mole}=6.82moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{18.2g}{1g/mole}=18.2moles$

• 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 6.82 moles.

For Carbon = $\frac{6.82}{6.82}=1$

For Hydrogen = $\frac{18.2}{6.82}=2.68\approx 3$

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

The ratio of C : H = 1 : 2

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