`N_2(g)+O_2(g)+181kJ leftrightarrow 2NO(g)` Write the Le Chatelier's conditions for shifting the equilibrium towards the formation of nitric acid.

N_2O_4(g) +57 KJ leftrightarrow 2NO_2(g) . Predict favourable Le chaterlier conditions.

0.482 mol N_2 and 0.933 mol O_2 are placed in a 10 L vessel and allowed to form N_2O at constant temperature. Numerical value of K_c for the reaction 2N_2(g)+O_2(g) leftrightarrow 2N_2O(g) is 2 times 10^-37 K mol^-1 . Calculate the equilibrium concentration of nirous oxide.

At 125^@C the K_p for the reaction N_2(g)+3H_2(g) leftrightarrow 2NH_3(g) is 2.15 times 10^-6 atm^-2 . Calculate K_c for the equilibrium at same temperature.

K_p for the reaction N_2O_4(g) leftrightarrow 2NO_2(g) at 750K is 640torr. Calculate the percentage of dissociation of N_2O_4 at equilibrium pressure of 160torr.

2SO_2(g) +O_2(g) leftrightarrow 2SO_3(g) IF the volume of reaction vessel is increased, what happens to Kc. Explain.

Comment on "N_2(g) + O_2(g) + Heat rarr 2NO(g) ' equation.

N_(2(g))+O_(2(g))rarr 2NO_(2(g))-Q is ……………..

For the gaseous reactions (I) and (II) the equilibrium constants are X and Y respectively. I. (1)/(2)N_(2)(g) + O_(2) (g) hArr NO_(2)(g) (II) 2NO_(2)(g) hArr N_(2)O_(4) (g) Using the above reactions the equilibrium constant Z for the reaction (III) given below is III. N_(2)O_(4)(g) hArr N_(2)(g) + 2O_(2) (g)

Consider the reaction cquilibrium, 2SO_(2(g)) + O_(2(g)) hArr 2 SO_(3(g)) , Delta H^(@) = - 198KJ . On the basis of Le Chatelier's principle, the condition favourable for the forward reaction is