Question

Sodium reacts with excess oxygen to form sodium oxide. A student wants to prepare 1.24g of sodium oxide. While doing the calculations, he uses atomic number of sodium instead of atomic mass. What is the approximate percentage error in the mass of sodium oxide obtained due to this mistake?

Answer 1

Answer:The approximate percentage error in the mass of sodium oxide obtained due to this mistake 36.97%.

Explanation:

$\text{Number of moles}=\frac{\text{given mass}}{\text{molecular mass}}$

Experimental value of number of moles $Na_2O$ when student used atomic number of sodium instead of atomic mass:

$n_1=\frac{1.24 g}{11\times 2+16}=0.0326 moles$

Actual value Number of moles $Na_2O$:

$n_2=\frac{1.24 g}{23\times 2+16}=0.0238 moles$

Percentage error = $=\frac{|\text{experimental value - theoretical value}|\times 100}{\text{theoretical value}}$

$\text{Percentage error}=\frac{|n_1-n_2|\times 100}{n_2}=\frac{|0.0326 moles-0.0238 moles|\times 100}{0.0238}=36.97\%$

The approximate percentage error in the mass of sodium oxide obtained due to this mistake 36.97%.

Answer 2

Answer:60 percent

Explanation: