Consider the following equilibrium at 461.9 K: NH4HS(s) ⇆ NH3(g) + H2S(g) The partial pressure of each gas is 0.287 atm. Calculate KP and Kc for the reaction.

Question

The answer should be in scientific notation.

Answer 1

Kp=P_NH3P_H2S

Kp=(0.287)(0.287)

Kp=0.0824=8.24•10^-2

Kp=Kc(RT)^Δn

Δn=(moles gas product)-(moles gas reactant)

Δn=2-0=2

R=0.08206 ^L•atm/_mol•K

T=461.9K

0.0824=Kc(0.08206×461.9)²

Kc=0.000057355 = 5.74•10^-5