Answer:
The equilibrium constant in terms of concentration that is, 
.
Explanation:
The relation of 
is given by:
= Equilibrium constant in terms of partial pressure.=98.1
= Equilibrium constant in terms of concentration =?
T = temperature at which the equilibrium reaction is taking place.
R = universal gas constant
= Difference between gaseous moles on product side and reactant side=
The equilibrium constant in terms of concentration that is, .
There is a very simple relationship between the three. First off, power is the amount of energy used over a certain amount of time. Energy is the capacity of carrying out that power. Lastly, time depends on how much energy you have to exert the work.
Hope this helps :)
Answer:
I. Increasing pressure will allow more frequent successful collision between particles due to the particles being closer together.
II. Rate of reaction increases due to more products being made; as increased pressure favours the exothermic side of the equilibrium.
III. Increasing temperature provides particles lots of (Kinetic) energy, for more frequent successful collision due to the particles moving at a faster rate than before. However, favouring the endothermic side of the equilibrium due to lots of energy required to break and form new bonds.
IV. Rate of reaction increases due to increase temperature favouring both directions of the equilibrium - causing products to form faster.
Hope this helps!
