1.
CH4 + 2H2S <--> CS2 +4H2
initial:
0.5
0.75
0 0
at equilibrium:
0.5-x
0.75-2x
x 4x
Given that equilibrium concentration of H2= 0.44 M
so, 4x = 0.44 M
x = 0.44/4 = 0.11 M
At equilibrium concentration of various species are:
[CH4] = 0.5-x = 0.5 - 0.11 = 0.39 M
[H2S] = 0.75 -2x = 0.75 - 2*0.11 = 0.53 M
[CS2] = x = 0.11 M
[H2]= 4x = 4*0.11 =0.44 M
Kc = [H2]^4 * [CS2] / [CH4] [H2S]^2
= (0.44)^4 *(0.11) /(0.39)*(0.53)^2
= 0.0376
Ans: 0.0376
2.
Equilibrium constant expression of Kc will be:
Kc= [P4O10] / {[P4]*[O2]^5}
Sinceconcentration of solid doesn't change, we can write Kc as:
Kc= 1/ [O2]5
= [O2]-5
Name: Date: CHE 112L Pre-Lab Assignment Experiment # 2: "Equilibrium Constant for a Chemical Reaction" Assignment...
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