Equilibrium

for a given reversible reaction depends only on temperature

. Adding inert gas at constant volume will not affect partial pressure of reactant or products, hence will not affect equilibrium amount o f either reactant or products.

As the number of moles of products and reactants are equal, so equilibrium constant is not affected by any change in pressure and volume. Catalyst also does not affect the equilibrium constant. It is an endothermic reaction, hence equilibrium constant depends only upon the temperature.

pH =

kcal
The above reaction is exothermic, increasing temperature will favour backward reaction, will increase the amount of .
Decreasing pressure will favour reaction in direction containing more molecules (reactant side in the present case). Therefore, decreasing pressure will increase amount of .
Removing , which is a reactant, will favour reaction in backward direction, more will be formed.
Adding will favour backward reaction and some of the will be dehydrogenated to .

The reaction of HA with strong base is

K =
=

In reactions (a), (b) and (c), atleast one of the product is either insoluble precipitate or a gas that drive the reaction continuously to right and do not allow equilibrium to be established. Following is the reversible reaction

exist in polymeric forms and has no electron deficiency, not a Lewis acid.

and are in so lid state, changing their a mount has no effect on equilibrium . Increasing temperature will favour forward reaction due to endotherm ic nature of reaction. Also, increasing pressure will favour backward reaction in which some (g ) w ill com bine with forming

Adding reactant will drive the reaction in forward direction in order to restore equilibrium. Therefore, addition of CO (g) will increase the equilibrium amount of C .

Both temperature and pressure will change the equilibrium amount of (g). Temperature changes the value of equilibrium constant.

= Buffer solution

If HCl is taken in limited quantity, final solution will have both and needed for buffer solution.
Ammonia and ammonium chloride forms basic buffer

As time passes, amount of products 'C' and 'D' increases,
hence Q increases.

is function of temperature only, does not
change with either p or x.

At constant temperature, having the volume will change both p and remains constant.

Minimum concentration would be required for precipitation of least soluble HgS.
For HgS, required for precipitation is
M

% hydrolysis = 100 =0.01

mmol of base = 2.5
mmol of acid required to reach the end point = 1
Volume of acid required to reach the end point =
Total volume at the end point = ml.
Molarity of salt at the end point =


10

MX :



Order of solubility is

In combination, if
is present in limiting amount, it will be neutralised
completely, leaving behind some excess of

PLAN In presence of common ion (in this case ion) solubility of
sparingly soluble salt is decreased.
Let solubility of in presence of 0.1 M



Total [ | = (2v + 0.1) M = 0.1 M
as x <<< 0.1 M
[
Thus,

x = 1. 1 M

M
p H = 2 M
For dilution of HCl,

L
Volume of water to be added = 10 - 1 = 9 L

PLAN Heat of reaction is dependent on temperature (Kirchhoff's equation) in heterogeneous system, equilibrium constant is independent on the molar concentration of solid species. Heat of reaction is not affected by catalyst. It lowers activation energy. By KirchhofFs equation, varies with temperature. Thus, (a) is correct. K is dependent on pressure of but independent of molar concentration of , Thus, (b) and (c) are correct. At a given temperature, addition of catalysis lowers activaion energy, H remaining constant. Thus, (d) is also correct. = Activation energy in absence of catalyst ' = Activation energy in presence of catalyst

Initially larger is the temperature greater is the yield but due to exothermic reaction as the time lapse yield become less.

The compressibility factor (Z) =
L/mol

y = 0.8 L/mol
Using the equation PV = nRT,
P =
x = 80 atm