The two common chlorides of phosphorus, pcl3, and pcl5, both important for the production of the other phosphorus compounds, coexist in equilibrium through the reactionpcl3(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 ?

(a) Kc = 264

(b) Kp = 6.15

Explanation:

(a) To calculate Kc we need the molar concentrations of each substance.

Then, we replace these concentrations in the Kc expression.

(b) To find out Kp we can use the following expression:

where,

R is the ideal gas constant (0.08206 atm .L /mol . K)

T is the absolute temperature (250°C + 273.15 = 523.15 K)

Δn is gaseous moles of products - gaseous moles of reactants (1 - 2 = -1)

If we replace with the values we have:

the right answer is c i just did the question.