`N_2O_4` is `66%` dissociated into `NO_2` at 340 K and 1 atm pressure. Find the volume occupied by 10 g `N_2O_4`, under these condition.

N_2O_4 is dissociated to 33% and 40% at total pressures P_1 and P_2 atm respectively. Hence, the ratio of P_1 to P_2 is

2 volumes of O_(3) produce 3 volumes of O_(2) on complete decomposition. 40 mL of a mixture of O_(3) and O_(2) is heated at first and then brought back to the previous temperature and pressure. The volume of the gaseous mixture is now found to be 42 mL. find the percentage composition of O_(3) in the gas mixture by volume. the volume of all gases are measured under the same conditions of temperature and pressure.

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_2O_4 (g) overset(rightarrow)(leftarrow)2NO_2 (g) at equilibrium the degree of dissociation (alpha) is 28% at temperature 318 K and total pressure 2 atm. Calculate the K_P and K_C for the reaction.

What volume of gas will be formed at 523 K and 1 atm pressure by the explosive decomposition of 5 g of the ammonium nitrate, according to the given equation? 2NH_(4)NO_(3)(s)=2N_(2)(g)+O_(2)(g)+4H_(2)O(g)

A two litre vessel contains 4 moles of N_2O_5 . On heating to 100^@C, N_2O_5 undergoes complete dissociation to NO_2 and O_2 . Mark out the correct inference (s) if rate constant for decomposition of N_2O_5 is 5.2xx10^-4 sec^-1

The value of K_p for the reaction 2H_2O(g) +2Cl_2(g) iff 4HCl(g) +O_2(g), is 0.035 atm at 400^@C , when the partial pressure are expressed in atmosphere. Calculate the value of K_c for the same reaction.