A sample of NH4HS(s) is placed in a 2.57 −L flask containing 0.140 mol NH3(g).
NH4HS(s)⇌NH3(g)+H2S(g)KP=0.108at25∘C
What will be the total gas pressure when equilibrium is established at 25∘C?
any idea on how to solve it like an outline?
Thanks
Use PV = nRT and solve for pNH3 initially. Substitute pNH3 from this calculation into the below.
pNH3 is approx 1.5 but you need a more accurate number.
...........NH4HS ⇌ NH3 + H2S
I.........solid....1.5....0
C.........solid.....+x....x
E.........solid....1.3+x...x
Substitute the E line into the Kp expression and solve for x, then evaluate 1.5(or whatever that number is) +x
Ptotal = pNH3 + pH2S
To solve this problem and determine the total gas pressure when equilibrium is established at 25∘C, you can follow these steps:
1. Set up the balanced chemical equation: NH4HS(s) ⇌ NH3(g) + H2S(g)
2. Use the given value of KP (equilibrium constant) = 0.108.
3. Calculate the initial pressure of NH3(g). Since you are given the number of moles (0.140 mol) and the volume of the flask (2.57 L), you can use the ideal gas law equation (PV = nRT) to find the initial pressure of NH3(g).
4. To determine the equilibrium pressures of NH3(g) (P(NH3)) and H2S(g) (P(H2S)), you need to make use of the equilibrium constant (KP). The equilibrium pressures are related to the initial pressure of NH3(g) and the equilibrium constant according to the equation: KP = (P(NH3) * P(H2S)) / (P(NH4HS)). Rearrange this equation to solve for P(NH4HS) using the given value of KP and the calculated pressure of NH3(g).
5. Sum up the equilibrium pressures of NH3(g) and H2S(g) to calculate the total gas pressure.
By following these steps, you will be able to determine the total gas pressure when equilibrium is established at 25∘C.