Chemistry: How many ions are found in 7.39 g of methanol?

How many ions are found in 7.39 g of methanol?

lufung8627

29.09.2020

Thus empirical and molecular formula is sa,e for C_4H_8O

Explanation:

Molecular formula is the chemical formula which depicts the actual number of atoms of each element present in the compound.

Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.

1. The empirical formula is CO_2H

The empirical weight of CO_2H = 1(12)+2(16)+1(1)= 45g.

The molecular weight = 90 g/mole

Now we have to calculate the molecular formula:

$n=\frac{\text{Molecular weight }{\text{Equivalent weight}=\frac{90}{45}=2$

The molecular formula will be= $2\times CO_2H=C_2O_4H_2$

2. The empirical formula is CH_3O

The empirical weight of CH_3O = 1(12)+3(1)+1(16)= 31 g.

The molecular weight = 62 g/mole

Now we have to calculate the molecular formula:

$n=\frac{\text{Molecular weight }{\text{Equivalent weight}=\frac{62}{31}=2$

The molecular formula will be= $2\times CH_3O=C_2H_6O_2$

3. The empirical formula is C_2H_4O

The empirical weight of C_2H_4O = 2(12)+4(1)+1(16)= 44 g.

The molecular weight = 88 g/mole

Now we have to calculate the molecular formula:

$n=\frac{\text{Molecular weight }{\text{Equivalent weight}=\frac{88}{44}=2$

The molecular formula will be= $2\times C_2H_4O=C_4H_8O_2$

4. The empirical formula is C_4H_8O

The empirical weight of C_4H_8O = 4(12)+8(1)+1(16)= 72 g.

The molecular weight = 72 g/mole

Now we have to calculate the molecular formula:

$n=\frac{\text{Molecular weight }{\text{Equivalent weight}=\frac{72}{72}=1$

The molecular formula will be= $1\times C_4H_8O=C_4H_8O$

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