Chemical Equilibrium
Hey it's me again! I have a question about chemical equilibrium.
At temperatures near 400 C, the Kp value for the synthesis of ammonia is 2.5 x 10-4. At 400 C, what would be the approximate value of K for the following reaction?
3H2(g) + N2 (g)⇔ 2NH3 (g)
So, the equation for the partial pressure is Kp = Kc(RT)Δn
Δn-2-4= -2
To solve for Kc, it's Kc= Kp/RTΔn
so it's Kc= 2.5 x 10-4 / (0.821 L atm/Kmol x 673.15 K)-2
Only I get a different answer than what's in the book.
Can anyone tell me where I went wrong? Thanks!
At temperatures near 400 C, the Kp value for the synthesis of ammonia is 2.5 x 10-4. At 400 C, what would be the approximate value of K for the following reaction?
3H2(g) + N2 (g)⇔ 2NH3 (g)
So, the equation for the partial pressure is Kp = Kc(RT)Δn
Δn-2-4= -2
To solve for Kc, it's Kc= Kp/RTΔn
so it's Kc= 2.5 x 10-4 / (0.821 L atm/Kmol x 673.15 K)-2
Only I get a different answer than what's in the book.
Can anyone tell me where I went wrong? Thanks!