Question

If molecular weight of glucose-1-phosphate is 260 and its density is 1.5g cm−3 ,what is the average volume occupied by 1 molecule of this compound ?

Answer 1

d = m/v
1.5 = 260/v
v = 260/1.5 = 173.33 cm^3

volume occupied by 1 molecule of this compound will be 173.33 cm^3

Answer 2

Answer: The average volume occupied by 1 molecule will be $9.579\times 10^{-27}cm^3$

Explanation:

To calculate the volume of 1 molecule, we use the formula for calculating the density and then divide the answer with Avogadro's number.

$Density=\frac{Mass}{Volume}$

Mass of glucose-1-phosphate = 260g/mol

Density of glucose-1-phosphate = $1.5g/cm^3$

Volume of glucose-1-phosphate = ?

Putting values in above equation, we get:

$1.5g/cm^3=\frac{260g/mol}{Volume}\\\\Volume=5.769\times 10^{-3}cm^3/mol$

Now, to calculate the volume of 1 molecule, we divide the volume by Avogadro's Number, we get:

$\text{Average volume}=\frac{5.769\times 10^{-3}cm^3/mol}{6.022\times 10^{23}mol^{-1}}\\\\\text{Average volume}=0.957\times 10^{-26}cm^3=9.579\times 10^{-27}cm^3$

Hence, the average volume occupied by 1 molecule will be $9.579\times 10^{-27}cm^3$