`4NH_(3)(g)+5O_(2)(g)hArr 4NO(g)+6H_(2)O(g)`. Write the `K_(p) and K_(c)` values for the above reaction and also make a relation between them.

(i) 4Nh_3(g) + 5O_2 (g) s iff 4NO (g) + 6H_2O (g) . Write the K_p and K_c values for the above reaction and also make a relation between them.

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

Find out the value of equilibrium constant, for the reaction, 2NH_(3)(g)+(5)/(2)O_(2)(g)hArr2NO(g)+3H_(2)O(g) . Consider K_(1),K_(2) and K_(3) as the respective equilibrium constants of the given three reaction: N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g) . . . (1) N_(2)(g)+O_(2)(g)hArr 2NO(g) . . (2) H_(2)(g)+(1)/(2)O_(2)(g)hArr H_(2)O(g) . . . (3)

For the reaction 4NH_(3)(g)+5O_(2)(g)rarr4NO(g)+6H_(2)O(g) write the instantaneous reaction -rate in terms of decrease in concentration of the reactants and increase in the concentration of the products.

The equilibrium constant of the following equilibria SO_(2)(g)+(1)/(2)O_(2)(g)hArr SO_(3)(g) 2SO_(3)(g)hArr 2SO_(2)(g)+O_(2)(g) are given by K_(1) and K_(2) respectively. Find the relation between K_(1) and K_(2) .

Given: C_(3)H_(8)(g)+5O_(2)(g)to3CO_(2)(g)+4H_(2)O(l) and C_(3)H_(8)(g)+5O_(2)(g)to3CO_(2)(g)+4H_(2)O(g) . At a fixed temperature and pressure between these two reactions the heat evolved in the second reaction is _____ than that in the first one.

For the reaction , 4NH_(3)(g)+5O_(2)(g)rarr4NO(g)+6H_(2)O(g) the concentration of NO increases to 0.18"mol.L"^(-1) in 5s. Calculate the rate of the reaction during that period of time

For the reaction , 4NH_(3)(g)+5O_(2)(g)rarr4NO(g)+6H_(2)O(g) the concentration of NO increases to 0.18"mol.L"^(-1) in 5s. Calculate rate of formation of water

Write the expressions of K_(c) and K_(p) for the reaction: 3O_(2)(g)hArr2O_(3)(g) .