Mustard gas, S(CH2CH2Cl)2 can be made at room temperature as shown:
SCl2(g) + 2 C2H4(g) <=> S(CH2CH2Cl)2(g)
In a particular experiment, 0.459 M of SCl2 and 0.919 M C2H4 were mixed. At equilibrium, [S(CH2CH2Cl)2(g)] was 0.141 M.
Calculate the value of Kc for the reaction.
Give your answer to 3 significant figures.
The answer is 1.09 but I dont know how to get it. can someone help me?
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Verified answer
Prepare an ICE chart following the concentrations of each species during the reaction.
Molarity . . . . . .SCl2(g) + 2 C2H4(g) <=> S(CH2CH2Cl)2(g)
Initial . . . . . . . .0.459 . . . . 0.919 . . . . . .. . . . . .0
Change . . . . . . .-x . . . . . . .-2x . . . . . . . . . . . . x
Equilibrium . . .0.459-x . . .0.919-2x . . . . . . . . . .x
But we are told that at equilibrium, [S(CH2CH2Cl)2] = 0.141 M = x
[SCl2] = 0.459 - x = 0.459 - 0.141 = 0.318 M
[C2H4] = 0.919 - 2x = 0.919 - (2)(0.141) = 0.637 M
Kc = [S(CH2CH2Cl)2] / [SCl2][C2H4]^2 = (0.141) / (0.318)(0.637)^2 = 1.09
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