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Masschaos
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A 9g sample of solid NH4Cl is heated in a 4L container to 924.4oC and decomposes according to the following equation.
NH4Cl(s) -> HCl(g) + NH3(g)
at equalibrium the partial pressure of NH3 (g) is 1.346 atm. Calculate the equilibrium constant for Kp for this reaction
Kp = Pproductn/Preactantn
or
Kc equation and Pv = nRT
First I used the Ideal gas equation the amount of NH3 in the system.
So n = PV/RT
n = (136383.45 Pa * (4 *10-3 L))/(8.3144*1197.4K)
n = 5.48*10-5
This means the concentration of the NH4Cl is.
n = 9/54.45 = 0.1653
0.1653 - 2(5.48*10-5) = 0.1652
I assumed then that Cl would also have this concentration.
So the Kc of the reaction = ([5.48*10-5*[5.48*10-5)/0.1652 = 1.817 * 10-8
Then Kp = Kc(RT)(delta)n
Kp= 1.817 * 10-8 * (8.3144*1197.4K)1
Kp = 0.00018 = 1.8*10-4
The more I look at this the more I feel there is a much easier solution, is my solution even right?
NH4Cl(s) -> HCl(g) + NH3(g)
at equalibrium the partial pressure of NH3 (g) is 1.346 atm. Calculate the equilibrium constant for Kp for this reaction
Homework Equations
Kp = Pproductn/Preactantn
or
Kc equation and Pv = nRT
The Attempt at a Solution
First I used the Ideal gas equation the amount of NH3 in the system.
So n = PV/RT
n = (136383.45 Pa * (4 *10-3 L))/(8.3144*1197.4K)
n = 5.48*10-5
This means the concentration of the NH4Cl is.
n = 9/54.45 = 0.1653
0.1653 - 2(5.48*10-5) = 0.1652
I assumed then that Cl would also have this concentration.
So the Kc of the reaction = ([5.48*10-5*[5.48*10-5)/0.1652 = 1.817 * 10-8
Then Kp = Kc(RT)(delta)n
Kp= 1.817 * 10-8 * (8.3144*1197.4K)1
Kp = 0.00018 = 1.8*10-4
The more I look at this the more I feel there is a much easier solution, is my solution even right?