Consider the reaction :
`1/2 N_2+O_2 hArr NO_2` + Heat
What is the effect of the following on the equilibrium:
(i)decrease in temperature
(ii)increase in volume
(iii) addition of `N_2`
(iv) decrease in concentration of `O_2` ?

Consider the reaction : 2SO_2(g)+O_2(g) hArr 2SO_3(g) +189.4 kJ . Indicate the direction in which the equilibrium will shift when (i)temperature is increased (ii) volume is increased (iii) a catalyst is added (iv) pressure is decreased (v) concentration of SO_2 is increased (vi) helium gas is added at constant volume so that the total pressure is increased (vii) helium gas is added at constant pressure.

Consider the following reaction N_(2)O_(4)(g)hArr2NO_(2)(g)DeltaH=58.6KJ What will be the effect of the following changes on the concentration of N_(2)O_(4) at equilibrium? (i) Increasing the pressure (ii) Increasing the temperature (iii) Increasing the volume (iv) Adding more NO_(2)(g) to the system without changing temperature and pressure (v) Adding catalyst.

N_(2) + 3H_(2)hArr2NH_(3) If temperature of following equilibrium reaction increases, then the reaction

For the reaction N_(2)O(g) hArr 2NO_(2)(g). DeltaH=57.49kJ // mole, the vapour density of equilibrium mixture ……………………….. with increase of temperature.

N_2O_4(g) hArr 2NO_2(g) . In this reaction, NO_2 is 20% of the total volume at equilibrium. Calculate (a) vapour density. (b) percentage dissociation of N_2O_4 .

What is the effect of decreasing the volume of the container in the reaction. 2C(s) + O_(2)(g) ltimplies 2CO(g)