If Kp For This Reaction Is 0.071 At 100 °C (when The Partial Pressures Are Measured In Atmospheres), What Is The Total Pressure In The Flask At Equilibrium? Total Pressure = Atm.

Here is the full question:

Ammonium iodide decomposes on heating.

NH₄I(s) ⇄ NH₃(g) + HI(g)

If Kp for this reaction is 0.071 at 100 °C (when the partial pressures are measured in atmospheres), what is the total pressure in the flask at equilibrium?

Total pressure = atm

0.53292 atm

Explanation:

Given that:

= 0.071   at 100°C

At equilibrium:

=  

=

0.071 = x²

x =

x = 0.26646 atm

Total Pressure =

Total Pressure = (0.26646) + (0.26646)

Total Pressure = 0.53292 atm

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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