Chemical EquilibriumHard

Question

A quantity of 34 g sample of BaO2 is heated to 1000 K in a closed and rigid evacuated vessel of 8.21 L capacity. What percentage of peroxide is converted into oxide? (Ba = 138)

2BaO2(s) $\rightleftharpoons$2BaO(s) + O2 (g); KP = 0.5 atm

Options

A.20%
B.50%
C.75%
D.80%

Solution

2BaO2(s) $\rightleftharpoons$2BaO(s) + O2(g)

$\frac{34}{170}\text{mole = 0.2}$

Equilibrium 0.2$x$ $x$ $\frac{x}{2}$

Now, $K_{p} = P_{O_{2}} \Rightarrow 0.5 = \frac{\frac{x}{2} \times 0.0821 \times 1000}{8.21}$

⇒ $x$ = 0.1

∴% of BaO2 decomposed = $\frac{0.1}{0.2} \times 100 = 50\%$

Create a free account to view solution

View Solution Free
Topic: Chemical Equilibrium·Practice all Chemical Equilibrium questions

More Chemical Equilibrium Questions

Solid ammonium carbamate dissociates as: NH2COONH4(s) $\rightleftharpoons$2NH3(g) + CO3(g). In a closed vessel, solid am...For the reaction H2(g) + I2(g) $\rightleftharpoons$2HI(g), the value of equilibrium constant is 9.0. The degree of disso...The equilibrium constant for the reaction 3C2H2 $\rightleftharpoons$C6H6 is 4.0 at T K. If the equilibrium concentration...For NH4HS(s) ⇋ NH3(g) + H2S(g) ; observed pressure for reaction mixture at equilibrium is 1.12 atm at 106oC. The v...For the reaction SO2(g) + O2(g) ⇋ SO3(g), if KP = KC(RT)x where the symbols have usual meaning then the value of x...