Reaction between `N_(2) and O_(2)` takes place as follows: `2N_(2)(g)+O_(2)(g) hArr 2N_(2)O(g)`. If a mixture of 0.482 mol of `N_(2)` and 0.933 mol of `O_(2)` is placed in a 10 L reaction vessel and allowed to form `N_(2)O` at a temperature for which `K_(c)=2.0xx10^(-37)`, determine the composition of equilibrium mixture.

The relation between K_(p) and K_(c) for the following reaction : 2 SO_(2) (g) + O_(2) (g) hArr 2 SO_(3) (g) is -

Find the relation betweenn K_(p)&K_(c) for the given reactions: (1)/(2)N_(2)(g)+O_(2)(g)hArrNO_(2)(g)

Comment on the validity of Boyle's law for the following reaction: N_(2)O_(4)(g)hArr 2NO_(2)(g) .

Write the rate law of 2N_(2)O_(5(g))rarr 4NO_(2(g))+O_(2(g)) reaction.

For the equilibrium N_2 (g) + O_2(g) = 2 NO (g)

Discuss the rate of the reaction 2N_(2)O_(5(g)) rarr 4NO_(2(g))+O_(2(g))

A sample of air consisting mainly of N_2 and O_2 is heated at 2500K till the given equilibrium attains- N_2(g) + O_2 (g) hArr 2NO(g) . If the value of equilibrium constant (K_c) at this temperature is 2.1xx10^(-3) and the percentage of number of moles of NO(g) in the above equilibrium mixture is 1.8 %, then what will be the mole fractions of N_2 and O_2 in the sample of air used'?

A mixture of N_(2) and O_(2) at 1 bar pressure contains 80% N_(2) by weight. Calculate the partial pressure of N_(2) in the mixture.

The equilibrium constant (K_c) for the reaction N_2(g) + O_2(g) rarr 2NO (g) at temperature T is 4 xx 10^-4 . The value of K_c for the reaction NO(g) rarr 1/2 N_2(g) + 1/2 O_2(g) at the same temperature is