Home
Class 11
CHEMISTRY
The decomposition of N(2)O(4) to NO(2) i...

The decomposition of `N_(2)O_(4)` to `NO_(2)` is carried out at `280^(@)C` in chloroform. When equilibrium is reached, `0.2` mol of `N_(2)O_(4)` and `2xx10^(-3)` mol of `NO_(2)` are present in a `2L` solution. The equilibrium constant for the reaction
`N_(2)O_(4) hArr 2NO_(2)` is

Promotional Banner

Similar Questions

Explore conceptually related problems

The decompsotion of N_2O_4 to NO_2 is carried out at 280K in chloroform.When equilibrium is reached,0,2 mol of N_2O_4 and 2xx 10^(-3) mol of NO_2 are present in 2 litre solution .The equilibrium constant for the reaction, N_2O_4 hArr 2 NO_2 is

The decomposition of N_(2)O_(4) to NO_(2) is carried out at 280^(@)C . When equilibrium is reached, 0.2 mol of N_(2)O_(4) and 2xx10^(-3)" mol of "NO_(2) are present in 2 litres solution. The K_(C) for the reaction N_(2)O_(4)hArr 2NO_(2) is

The decomposition of N_(2)O_(4) to NO_(2) is carried out at 280^(@)C . When equilibrium is reached, 0.2 mol of N_(2)O_(4) and 2xx10^(-3)" mol of "NO_(2) are present in 2 litres solution. The K_(C) for the reaction N_(2)O_(4)hArr 2NO_(2) is

The dissociation of N_(2)O_(4) to NO_(2) was carried out at 298 K in chloroform medium. When equilibrium was reached, 0.2 mol of N_(2)O_(4) and 0.02 mol of NO_(2) were found to be present in a 2L solution. The K_(c) of the reaction at this temperature is

The equilibrium constant for the reaction NH_(4)NO_(2)(s)hArr N_(2)(g)+2H_(2)O(g) , is given by

Density of equilibrium mixture of N_(2)O_(4) and NO_(2) at 1 atm and 384 K is 1.84 g dm^(-3) . Calculate the equilibrium constant of the reaction. N_(2)O_(4)hArr2NO_(2)