The partial pressures of `N_(2)O_(4) "and" NO_(2) "at" 40^(@)C` for the following equilibrium `N_(2)O_(4)(g)hArr2NO_(2)(g)` are `0.1 "atm and" 0.3` atm respectively. Find `K_(P)` for the reaction.

For the equilibrium N_(2)O_(4(g))hArr 2NO_(2(g)) , the K_(p) and K_(c ) values are related as

For the equilibrium N_(2)O_(4(g))hArr 2NO_(2(g)) , the K_(p) and K_(c ) values are related as

For the equilibrium N_(2)O_(4(g))hArr 2NO_(2(g)) , the K_(p) and K_(c ) values are related as

K_p for the reaction : N_2O_4(g) hArr 2NO_2(g) is 0.157 atm at 27^@C and 1 atm pressure . Calculate K_c for the reaction.

The temperature at which K_(c) and K_(p) will have the same value for the equilibrium , N_(2) O_(4) (g) hArr 2 NO_(2) (g) is

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 ?

For the reaction, N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) the partial pressure of N_(2) and H_(2) are 0.80 and 0.40 atmosphere, respectively, at equilibrium. The total pressure of the system is 2.80 atm. What is K_(p) for the above reaction?

For the reaction, N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) the partial pressure of N_(2) and H_(2) are 0.80 and 0.40 atmosphere, respectively, at equilibrium. The total pressure of the system is 2.80 atm. What is K_(p) for the above reaction?