For the equilibrium:
NH4HS(s) ⇌ NH3(g) + H2S(g) How does Kp compare to Kc?
Kp > Kc
Kp = (Kc)1/2
Kp < Kc
Kp = (Kc)2
Kp = Kc
Kp = Kc(RT)^delta n where delta n = moles products - mols reactants
Look up Kp or Kc on the web and calculate the other, then compare Kp with Kc.
Kp and Kc like to play hide and seek with each other. Sometimes they're the same, sometimes they're different, and they love to keep chemists guessing. In this case, Kp and Kc are not the same crazy kids. So, the correct answer is Kp > Kc. It's like Kp likes to show off with its big nose, while Kc prefers to keep it subtle. No hard feelings though, they're just different ways of expressing the same equilibrium constant.
For the equilibrium reaction NH4HS(s) ⇌ NH3(g) + H2S(g), Kp and Kc represent the equilibrium constants in terms of partial pressures (Kp) and molar concentrations (Kc), respectively.
To determine how Kp compares to Kc, we need to understand the relationship between the two. Kp and Kc are related by the ideal gas law, which states that the partial pressure of a gas is proportional to its molar concentration.
Mathematically, the relationship between Kp and Kc is given by the equation:
Kp = Kc(RT)Δn
Where R is the ideal gas constant, T is the temperature in Kelvin, and Δn is the difference in the number of moles of gaseous products and reactants.
In the case of the given equilibrium reaction, there are two moles of gaseous products (NH3 and H2S) and one mole of a solid reactant (NH4HS). Hence, Δn = 2 - 1 = 1.
Since Δn = 1, Kp = Kc(RT).
Therefore, we can conclude that Kp is equal to Kc for this equilibrium reaction. Hence, the correct answer is Kp = Kc.
To determine how Kp compares to Kc for the given equilibrium, we need to understand the relationship between Kp and Kc. Kp represents the equilibrium constant in terms of partial pressures, while Kc represents the equilibrium constant in terms of concentrations.
First, let's define Kp and Kc for the given equilibrium:
Kp = (P(NH3) x P(H2S)) / P(NH4HS)
Kc = [(NH3) x (H2S)] / (NH4HS)
To compare Kp to Kc, we can look at the expression for Kp in terms of Kc:
Kp = (P(NH3) x P(H2S)) / P(NH4HS)
= ((NH3)RT x (H2S)RT) / (NH4HS)RT
= (RT)^2 x [(NH3) x (H2S)] / (NH4HS)
= (RT)^2 x Kc
From this equation, we can see that Kp is equal to (RT)^2 multiplied by Kc.
Since (RT)^2 is a positive constant, Kp will have the same value as Kc. Therefore, the answer is Kp = Kc.