We know that the relationship between K c and K p is K p = K c (RT) Δn What would be the value of ∆ n for the reaction NH 4 Cl (s) ⇋ NH 3 (g) + HCl (g)

Question

Philoid · Accepted Answer

In the equation K_p = K_c (RT) ^Δn,∆n equals to the difference b/w the number of moles of gaseous products and gaseous reactants where, K_p and K_c are the Equilibrium constants at constant pressure and temperature respectively.

For the reaction NH₄ Cl (s) ⇋ NH₃ (g) + HCl (g)

The no. of moles of reactant is 1 ( 1 molecule of ammonium chloride involved) and the no. of moles of reactant is 2 ( ammonia and HCl )

Then ,∆n = (2 – 1 ) = 1.

We know that the relationship between Kc and Kp is Kp = Kc (RT)ΔnWhat would be the value of ∆n for the reactionNH4 Cl (s) ⇋ NH3 (g) + HCl (g)

We know that the relationship between K_c and K_p is K_p = K_c (RT)^Δn
What would be the value of ∆n for the reaction

NH₄ Cl (s) ⇋ NH₃ (g) + HCl (g)