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25-10-2022
Chemistry

Answered

a sample of solid ammonium chloride was placed in an evacuated chamber, and then heated causing it to decompose according to the following reaction: nh4cl(s) nh3(g) hcl(g) in a particular experiment the pressure of nh3(g) in the container was found to be 2.3 atm. calculate the value of kp for the decomposition of nh4cl(s) at this temperature.

Answer :

03-11-2022

The value of the Kp (equilibrium constant) of the reaction is 4.84.

First let us write the balanced chemical reaction of decomposition,

NH₄Cl(s) ⇔ NH₃(g) + HCl(g)

The initial pressure of the container is zero.

On reaching equilibrium, let us assume that the pressure of HCl and NH₃ is found to be x, while the equilibrium temperature is 2.3 atm.

We know,

Kp = P[NH₃]¹P[HCl]¹

Where,

P[NH₃] and P[HCl] is the pressure of the gases at equilibrium.

So, now putting all the values,

Kp = [x][x]

Kp = [x]²

Here, it is given that the equilibrium pressure is 2.3, so, we can put x = 2.3,

So, putting all the values,

Kp = [2.3]²

Kp = 4.84

Hence, the Kp value of the reaction is 4.84.

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