Question

A homogeneous ideal gaseous reaction $A{B}_{2\left(g\right)}\rightleftharpoons A_{\left(g\right)}+{2B}_{\left(g\right)}$ is carried out in a 25 litre flask at~${27}^{0}C$. The initial amount of $A{B}_2$ was 1 mole and the equilibrium pressure was 1.9 atm. The value of $K_p$ is $x\times {10}^{-2}$ . The value of x is ..... (Integer answer)

Answer 1

$A{B}_2\rightleftharpoons A+2B$

$1--$

$1-\alpha \alpha 2\alpha$

$=0.5350.4650.93$

$1.9\times 25=n_T\times 0.08206\times 300$

$n_T=1.93=1+2\alpha$

$\alpha =0.465$

$K_p=\frac{(\frac{0.465}{1.93}\times 1.9){(\frac{0.93}{1.93}\times 1.9)}^2}{(\frac{0.535}{1.93}\times 1.9)}$

$K_p=73\times {10}^{-2}at{m}^{2}x=73$