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

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.