Question

what is the difference between empherical and molecular formula? a compound contain 69.9% iron,30.1% Oxygen it's molar mass is 160g. what are empherical and molecular formula?​

Answer 1

$\huge\underline\bold\red{QᑌESTIOᑎ}$

What is the difference between empherical and molecular formula?

$\huge\underline\bold\red{ᗩᑎSᗯEᖇ}$

$\tt{Molecular \: Formula}$

A molecular formula is a chemical formula that provides the number of each type of atom in a molecule.

$\tt{Empirical \: Formula}$

An empirical formula is a chemical formula that tells you a simple, whole number ratio for the atoms in a molecule.

$\huge\underline\bold\red{QᑌESTIOᑎ}$

A compound contain 69.9% iron,30.1% Oxygen it's molar mass is 160g. what are empherical and molecular formula?

$\huge\underline\bold\red{ᗩᑎSᗯEᖇ} </p><p> </p><p>$

The iron oxide has 69.9% iron and 30.1% dioxygen by mass.

Thus, 100 g of iron oxide contains 69.9 g iron and 30.1 g dioxygen.

◻The number of moles of iron present in 100 g of iron oxide are

$\boxed {\frac{69.9}{55.8}}$

=1.25

→ The number of moles of dioxygen present in 100 g of iron oxide are

$\boxed{ \frac{30.1}{32}}$

=0.94

Therefore ,

Ratio of oxygen atom to no of carbon atom present in one formula unit of iron oxide is

$\tt \frac{2 \times 0.94}{1.25} = \frac{1.5}{1}</p><p>$

$\tt{1.252×0.94}$

$\tt{ = </p><p>1</p><p>1.5</p><p> }$

Ratio is 3 :1

Hence, the formula of the iron oxide is Fe²O³

Answer 2

$\huge\underline\bold\red{QᑌESTIOᑎ}$

What is the difference between empherical and molecular formula?

$\huge\underline\bold\red{ᗩᑎSᗯEᖇ}$

$\tt{Molecular \: Formula}$

A molecular formula is a chemical formula that provides the number of each type of atom in a molecule.

$\tt{Empirical \: Formula}$

An empirical formula is a chemical formula that tells you a simple, whole number ratio for the atoms in a molecule.

$\huge\underline\bold\red{QᑌESTIOᑎ}$

A compound contain 69.9% iron,30.1% Oxygen it's molar mass is 160g. what are empherical and molecular formula?

$\huge\underline\bold\red{ᗩᑎSᗯEᖇ} </p><p> </p><p>$

The iron oxide has 69.9% iron and 30.1% dioxygen by mass.

Thus, 100 g of iron oxide contains 69.9 g iron and 30.1 g dioxygen.

◻The number of moles of iron present in 100 g of iron oxide are

$\boxed {\frac{69.9}{55.8}}$

=1.25

→ The number of moles of dioxygen present in 100 g of iron oxide are

$\boxed{ \frac{30.1}{32}}$

=0.94

Therefore ,

Ratio of oxygen atom to no of carbon atom present in one formula unit of iron oxide is

$\tt \frac{2 \times 0.94}{1.25} = \frac{1.5}{1}</p><p>$

$\tt{1.252×0.94}$

$\tt{ = </p><p>1</p><p>1.5</p><p> }$

Ratio is 3 :1

Hence, the formula of the iron oxide is Fe²O³