Question

Convert the values of Kc to values of Kp or the values of Kp to values of Kc.

a) N₂(g)+3H₂(g) <--> 2NH₃(g); Kc=0.50 at 400 degrees Celsius.

b) H₂+I₂ <---> 2HI; Kc= 50.2 at 448 degrees Celsius.

c) Na₂SO₄*10H₂O(s) <---> Na₂SO₄(s)+10H₂O(g). Kp=4.08x10⁻25 at 25 degrees Celsius.

d) H₂O(l) <---> H₂O (g); Kp= 0.122 at 50 degrees Celsius.

Answer 1

The relationship between the equilibrium constants Kc and Kp for gaseous reactions depends on the change in the number of moles of gases and the temperature in Kelvin, using the equation Kp = Kc(RT)Δn.

Step-by-step explanation:

The equilibrium constant is represented in terms of concentrations (Kc) for reactions in solutions or in terms of partial pressures (Kp) for gaseous reactions. The relationship between these two forms of the equilibrium constant depends on the change in the number of moles of gas during the reaction and is given by the equation Kp = Kc(RT)Δn, where Δn is the change in moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.

For example, in the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), Kc is given as 0.50 at 400°C. To convert this to Kp, we would use the equation Kp = Kc(RT)Δn considering the temperature in Kelvin and the change in moles of gas (Δn = 2 - 4 = -2 in this case).

Similarly, to convert Kp to Kc for a reaction like Na₂SO₄·10H₂O(s) ⇌ Na₂SO₄(s) + 10H₂O(g) with a given Kp, we would use the inverse operation, considering the reverse change in moles of gas.