Asked by ami
When solid NH4HS is placed in a closed flask at 28 C, the solid dissociates according to the equation:
NH4HS(s) <=> NH3(g) + H2S(g)
The total pressure of the equilibrium mixture is 0.766 atm. Determine Kp at this temperature.
Choose one answer.
a. 0.147
b. 0.766
c. 0.587
d. 0.383
e. 1.53
NH4HS(s) <=> NH3(g) + H2S(g)
The total pressure of the equilibrium mixture is 0.766 atm. Determine Kp at this temperature.
Choose one answer.
a. 0.147
b. 0.766
c. 0.587
d. 0.383
e. 1.53
Answers
Answered by
DrBob222
NH4HS(s) <=> NH3(g) + H2S(g)
p = partial pressure.
Kp = pNH3 x pH2S
Since the total pressure is 0.766 atm, and the number of moles NH3 = number of moles H2S, won't the partial pressure of each gas be just 1/2 of the total pressure? Substitute into Kp and solve. Check my thinking.
p = partial pressure.
Kp = pNH3 x pH2S
Since the total pressure is 0.766 atm, and the number of moles NH3 = number of moles H2S, won't the partial pressure of each gas be just 1/2 of the total pressure? Substitute into Kp and solve. Check my thinking.
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