[" Problem "7.8],[13.8g" of "N_(2)O_(4)" was placed in a "1L" reaction "],[" vessel at "400K" and allowed to attain "],[" equilibrium "],[N_(2)O_(4)(g)rightleftharpoons2NO_(2)(g)]

13.8g of N_(2)O_(4) was placed in a 1L reaction vessel at 400K and allowed to attain equilibrium N_(2)O_(4)(g)hArr2NO_(2)(g) The total pressure at equilibrium was found to be 9.15 bar . Calcualate K_(c) , K_(p) and partial pressure at equilibrium.

13.8 g of N_(2)O_(4) was placed in a 1L reaction vessel at 400 K and allowed to attain equilibrium N_(2)O_(4) (g) hArr 2NO_(2)(g) The total pressuers at equilibrium was found to be 9.15 bar. Calculate K_(c), K_(p) and partial pressure at equilibrium.

13.8 g of N_(2)O_(4) was placed in 1 L reaction vessel at 400K and allowed to attain equilibrium : N_(2)O_(4) (g) hArr 2NO_(2)(g). the total pressure at equilibrium was found to be 9.15 bar. Calculate K_(c),K_(p) and partial pressure at equilibrium .

18.4 g N_(2)O_(4) was placed in 1 L vessel at 400 K and allowed to attain the following equilibrium N_(2)O_(4)(g) hArr 2NO_(2)(g) . IF the total pressure at equilibrium was 10.64 bar, approximate K_(p) is (R = 0.083 L bar K^(-1) mol^(-1) ) (Assume N_(2)O_(4), NO_(2) as ideal gases)

18.4 g of N_(2)O_(4) is taken in a 1 L closed vessel and heated till the equilibrium is reached. N_(2)O_(4(g))rArr2NO_(2(g)) At equilibrium it is found that 50% of N_(2)O_(4) is dissociated . What will be the value of equilibrium constant?

18.4 g of N_(2)O_(4) is taken in a 1 L closed vessel and heated till the equilibrium is reached. N_(2)O_(4(g))hArr2NO_(2(g)) At equilibrium it is found that 50% of N_(2)O_(4) is dissociated . What will be the value of equilibrium constant?