<u>Answer:</u>
<u>For a:</u> The value of
for the given reaction is 271.6
<u>For b:</u> The value of
for the reaction is 6.32
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For
:</u>
Given mass of
= 0.105 g
Molar mass of
= 208.24 g/mol
Putting values in equation 1, we get:

- <u>For
:</u>
Given mass of
= 0.220 g
Molar mass of
= 137.33 g/mol
Putting values in equation 1, we get:

- <u>For
:</u>
Given mass of
= 2.12 g
Molar mass of
= 71.0 g/mol
Putting values in equation 1, we get:

Volume of the flask = 25.0 L
For the given chemical equation:

The equation used to calculate concentration of a solution is:

The expression of
for above reaction follows:

We are given:
![[PCl_5]=\frac{5.04\times 10^{-4}mol}{25L}](https://tex.z-dn.net/?f=%5BPCl_5%5D%3D%5Cfrac%7B5.04%5Ctimes%2010%5E%7B-4%7Dmol%7D%7B25L%7D)
![[PCl_3]=\frac{1.60\times 10^{-3}mol}{25L}](https://tex.z-dn.net/?f=%5BPCl_3%5D%3D%5Cfrac%7B1.60%5Ctimes%2010%5E%7B-3%7Dmol%7D%7B25L%7D)
![[Cl_2]=\frac{0.029mol}{25L}](https://tex.z-dn.net/?f=%5BCl_2%5D%3D%5Cfrac%7B0.029mol%7D%7B25L%7D)
Putting values in above equation, we get:

Hence, the value of
for the given reaction is 271.6
Relation of
with
is given by the formula:

where,
= equilibrium constant in terms of partial pressure = ?
= equilibrium constant in terms of concentration = 271.6
R = Gas constant = 
T = temperature = 
= change in number of moles of gas particles = 
Putting values in above equation, we get:

Hence, the value of
for the reaction is 6.32