Enter your answer in the provided box. a united nations toxicologist studying the properties of mustard gas, s(ch2ch2cl)2, a blistering agent used in warfare, prepares a mixture of 0.675 m scl2and 0.973 m c2h4and allows it to react at room temperature (20.0°c): scl2(g) + 2 c2h4(g) ⇌ s(ch2ch2cl)2(g) at equilibrium,[s( ch2ch2cl)2] = 0.350 m. calculate .

Explanation:

First we have to use the ICE table to find the equilibrium concentrations:

I    0.675 M   0.973 M           0

C    -X               -2X               +X

E  0.675-X     0.973-2X          X

The equilibrium concentration is given by the problem:

X=0.35 M

Then we have to do the substractions:

=  0.325 M

= 0.273 M

= 0.35 M

With the equilibrium concentrations is posible to calculate Kc:

With the Kc value is posible calculate Kp using the equation:

Kp = Kc(RT)^(Δn)

Kp= Equilibrium Pressure constant

Kc= Equilibrium Concentration constant

R= 0.08206 L*atm/mol*K

T= Temperature

Δn=moles of products - moles of reactants

T= 25 ºC= 298.15 K

Δn = 1 mole of products - 3 moles of reactants = -2

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