Chemical EquilibriumHard
Question
Solid NH4HS dissociates into NH3 and H2S at a certain temperature, the equilibrium pressure is P atm. If now, NH3 is pumped into the system so that its partial pressure becomes P atm, then what will be the partial pressure (in atm) of H2S?
Options
A.0.5 P
B.0.25 P
C.0.33 P
D.0.67 P
Solution
NH4HS(s) $\rightleftharpoons$ NH3 (g) + H2S(g)
Equ. partial pressure $\frac{P}{2}$atm $\frac{P}{2}$atm
New Equ. partial pressure P atm P′ atm
Now, $\frac{P}{2} \times \frac{P}{2} = P \times P' \Rightarrow P' = 0.25\text{ P}$
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
KP for formation of ethane from hydrogen and ethylene is 5.5 × 1018 atm−1 and KP for formation of ethylene from hydrogen...The equilibrium constant for the reaction N2(g) + O2(g) $\rightleftharpoons$ 2NO(g) is K1 and the equilibrium constant f...XeF6 + H2O $\rightleftharpoons$ XeOF4 + 2HF; equilibrium constant = K1.XeO4 + XeF6 $\rightleftharpoons$ XeOF4 + XeO3F2; ...For the reaction I2(g) $\rightleftharpoons$2I(g), KC = 1.0 × 10−2 mol lit−1. What volume of the vessel should be taken s...van 't Hoff equations show the effect of temperature on equilibrium constants KC and KP. KP and KC varies with temperatu...