Question

1. If 4.000 grams of hydrogen peroxide is placed within a sealed 250 milliliter container at 500 K.

What is the pressure of the oxygen gas produced in atmospheres?

2

Answer 1

Molar mass of $H_2O_2= 34 \ g$

Moles of $H_2O_2= \frac{4}{34}$

$2H_2O_2\to 2H_2O + O_2$

So ,moles of oxygen produced will be half of hydrogen peroxide .

$n= \frac{2}{34}$

$T=500K,V= 250\ ml = 0.25 \ L$

Using ideal gas equation,

$PV= nRT$

$P\times 0.25= \frac{2}{34}\times 0.0821 \times 500\implies$

$P=9.66 \ atm$