The two common chlorides of phosphorus, pcl3, and pcl5, both important for the production of the other phosphorus compounds, coexist in equilibrium through the reaction
pcl3(g) + cl2(g) = pcl5(g)
at 250 ᵒc , an equilibrium mixture in a 25.0 l flask contains 0.105 g pcl5, 0.220 g pcl3 and 2.12 g of cl2. what are the values of
a) kc
b) kp for this reaction at 250 ᵒc ?

For a: The value of for the given reaction is 271.6

For b: The value of for the reaction is 6.32

Explanation:

To calculate the number of moles, we use the equation:

     .....(1)

Given mass of = 0.105 g

Molar mass of = 208.24 g/mol

Putting values in equation 1, we get:

Given mass of = 0.220 g

Molar mass of = 137.33 g/mol

Putting values in equation 1, we get:

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:

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

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

you gotta add the following molecules so we can give u an answer

explanation: