Answer:
Kp = 0.2215
Kc = 0.0052
Explanation:
<u>Step 1:</u> The balanced equation
PCl5(g) → PCl3(g) + Cl2(g)
<u>Step 2:</u> given data
Initial pressure PCl5 = 0.50 atm
Temperature = 523 Kelvin
The actual pressure in the flask was found to be 0.74 atm.
<u>Step 3:</u> Calculate the pressure after the decomposition
Pressure of PCl5 after decomposition = 0.5 - X
Since the equation has a ratio 1:1 the pressure after the decomposition of PCl3 and Cl2 is X
<u>Step 4:</u> Calculate total pressure at equilibrium
0.74 atm = 0.5 atm - X + 2X
X = 0.74 - 0.5 = 0.24 atm
<u>Step 5:</u> Calculate Kp
Kp = P(PCl3)* P(Cl2) / P(PCl5)
Kp = 0.24² / 0.26 = 0.2215
<u>Step 6:</u> Calculate Kc
The ideal gas wet: P*V = nRT
with P= the pressure of the gas in atm
with V= the volume of the gas in L
with n= the number of moles
with R= the gas constant in L*atm/mol*K
T = the temperature in Kelvin
P= nRT/V
Kp= Kc*(RT)^Δn
Kc=Kp/(RT)^Δn
Kc= 0.2215 / (0.08206*523)^1
Kc= 0.0052
