At 300K , the partial pressures of `N_2O_4`(g) and `NO_2`(g) in an equilibrium mixture of the reaction: `N_2O_4(g)

For the reaction, N_(2)O_(4)(g)hArr2NO_(2)(g) occurring in a closed vessel at 300K, the partial pressures of N_(2)O_(4)(g) and NO_(2)(g) at equilibrium are 0.28 atm and 1.1 atm respectively. What will be the partial pressures of these gases if the volume of the reaction system is doubled keeping the temperature constnt ?

At 46^@C, K_p for the reaction N_2O_4(g) iff 2NO_2(g) is 0.66. Calculate the partial pressure of N_2O_4 and NO_2 at equilibrium and at a total pressure of 0.5 atm.

N_(2)O_(3) is an unstable oxide of nitrogen and it decomposes into NO (g) and NO_(2)(g) where NO_(2)(g) is further dimerise dimerise into N_(2)O_(4) as N_(2)O_(3)(g)hArrNO_(2)(g)+NO(g)" ",K_(p_(1)=2.5 bar 2NO_(2)(g)hArrN_(2)O_(4)(g)" ": K_(P2) A flask is initially filled with pure N_(2)O_(3)(g) having pressure 2 bar and equilibria was established. At equilibrium partial pressure of NO (g) was found to be 1.5 ber. The equilibrium partial pressure of N_(2)O_(3)(g) is :

138 gm N_2O_4 is introduced into 8.21 litre container at 300 K. Temperature is increased to 600 K where it dissociates into NO_2 .If equilibrium partial pressure of N_2O_4 and NO_2 are equal than K_p (in atm ) for N_2O_4(g) hArr 2NO_2 at 600 K.

N_(2)O_(3) is an unstable oxide of nitrogen and it decomposes into NO (g) and NO_(2)(g) where NO_(2)(g) is further dimerise dimerise into N_(2)O_(4) as N_(2)O_(3)(g)hArrNO_(2)(g)+NO(g)" ",K_(p_(1)=2.5 bar 2NO_(2)(g)hArrN_(2)O_(4)(g)" ": K_(P2) A flask is initially filled with pure N_(2)O_(3)(g) having pressure 2 bar and equilibria was established. At equilibrium partial pressure of NO (g) was found to be 1.5 ber. The equilibrium partiaal pressure of N_(2)O_(3)(g) is :

N_(2)O_(3) is an unstable oxide of nitrogen and it decomposes into NO (g) and NO_(2)(g) where NO_(2)(g) is further dimerise dimerise into N_(2)O_(4) as N_(2)O_(3)(g)hArrNO_(2)(g)+NO(g)" ",K_(p_(1)=2.5 bar 2NO_(2)(g)hArrN_(2)O_(4)(g)" ": K_(P2) A flask is initially filled with pure N_(2)O_(3)(g) having pressure 2 bar and equilibria was established. At equilibrium partial pressure of NO (g) was found to be 1.5 ber. The equilibrium partiaal pressure of N_(2)O_(3)(g) is :