Here is the full question:
Ammonium iodide decomposes on heating.
NH₄I(s) ⇄ NH₃(g) + HI(g)
If Kp for this reaction is 0.071 at 100 °C (when the partial pressures are measured in atmospheres), what is the total pressure in the flask at equilibrium?
Total pressure = atm
Answer:
0.53292 atm
Explanation:
Given that:
[tex]K_p[/tex] = 0.071 at 100°C
At equilibrium:
[tex]K_p[/tex] = [tex][P_{NH_3}][P_{HI}][/tex]
[tex]K_p[/tex] = [tex][x][x][/tex]
0.071 = x²
x = [tex]\sqrt{0.071}[/tex]
x = 0.26646 atm
Total Pressure = [tex]P_{NH_3}}+ P_{HI}[/tex]
Total Pressure = (0.26646) + (0.26646)
Total Pressure = 0.53292 atm
