Answer:
The partial pressure of ammonia at the equilibrium is 0.00139 atm
Explanation:
Step 1: Data given
Kp = 1.47 * 10^-5
Temperature = 508 °C = 781 K
Partial pressure of H2 = 0.588 atm
Partial pressure of N2 = 0.645 atm
Step 2: The balanced equation
N2(g) + 3H2(g) ⇆ 2NH3(g)
Step 3: Calculate the partial pressure of ammonia
Kp = (pNH3)² / (pH2)³*(pN2)
⇒with Kp = 1.47 * 10^-5
⇒with pNH3 = the partial pressure of ammonia = TO BE DETERMINED
⇒with pH2 = the partial pressure of H2 = 0.588 atm
⇒with pN2 = the partial pressure of N2 = 0.645 atm
1.47 *10^-5 = (pNH3)² / ((0.588³)*(0.645))
(pNH3)² = 1.93 * 10^-6
pNH3 = 0.00139 atm
The partial pressure of ammonia at the equilibrium is 0.00139 atm
