NH4HS(s) ------------> NH3(g) + H2S(g)
I y 0 0
C -x +x +x
E y-x +x +x
at equilibrium PNH3 = PH2S = x
Kp = [NH3][H2S]
0.11 = x*x
x^2 = 0.11
x = 0.3316
PH2S = x = 0.3316atm
------ PCl5(g) -----------> PCl3(g) + Cl2(g)
I ----- 1.42 -------------- 0 -------- 0
C----- -x --------------- +x ----------- +x
E -----1.42-x ------------- +x --------- +x
Kp = PPCl3*PCl2/PPCl5
0.497 = x*x/(1.42-x)
0.497*(1.42-x) = x^2
x = 0.63
PPCl5 = 1.42-x = 1.42-0.63 = 0.79atm
PPCl3 = 0.63atm
PCl2 = 0.63atm
The squares in the equation are equilibrium signs. The equilibrium constant, Ky, for the following reaction...
The equilibrium constant, Ky, for the following reaction is 0.110 at 298 K. NH_HS(s) NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.50 L container at 298 K contains 2.94 mol of NH_HS(s) and 0.219 mol of NH3(g), the partial pressure of H2S(g) is atm.
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Practice Exercise 1 At 500 K, the reaction 2 NO(8) + Cl2(8) = 2 NOCI(8) has K, = 51. In an equilibrium mixture at 500 K, the partial pres- sure of NO is 0.125 atm and Cl, is 0.165 atm. What is the par- tial pressure of NOCI in the equilibrium mixture? (a) 0.13 atm (b) 0.36 atm (c) 1.0 atm (d) 5.1 x 10-5 atm (e) 0.125 atm Practice Exercise 2 At 500 K, the reaction PC15(8) = PC13(8) + Cl2(8) has...
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