Answer: The reaction is not at equilibrium and will proceed to make more products to reach equilibrium.
Explanation:
Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as 
K is the constant of a certain reaction when it is in equilibrium, while Q is the reaction quotient of activities of products and reactants at any stage other than equilibrium of a reaction.
For the given chemical reaction:
The expression for 
is written as:
![Q=\frac{[HI]^2}{[H_2]^1[I_2]^1}](https://tex.z-dn.net/?f=Q%3D%5Cfrac%7B%5BHI%5D%5E2%7D%7B%5BH_2%5D%5E1%5BI_2%5D%5E1%7D)
![Q=\frac{[0.0890]^2}{[0.215]^1[0.498]^1}](https://tex.z-dn.net/?f=Q%3D%5Cfrac%7B%5B0.0890%5D%5E2%7D%7B%5B0.215%5D%5E1%5B0.498%5D%5E1%7D)
Given : = 54.8
Thus as 
, the reaction will shift towards the right i.e. towards the product side.
To get the ans divide 5600by 78 and there is ur answer
Answer:
21.16 MPa
Explanation:
Partial pressure of oxygen = 5.62 MPa
Total gas pressure = 26.78 MPa
But
Total pressure of the gas= sum of partial pressures of all the constituent gases in the system.
This implies that;
Total pressure of the system = partial pressure of nitrogen + partial pressure of oxygen
Hence partial pressure of nitrogen=
Total pressure of the system - partial pressure of oxygen
Therefore;
Partial pressure of nitrogen= 26.78 - 5.62
Partial pressure of nitrogen = 21.16 MPa
