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

fire could start, buildings collapsing, and ash falling from the sky.

explanation:

this is because the buildings or plants could catch on fire and the buildings would most likely collapse. lastly ash would fall because all the burning would cause ash to fall from the sky.

hope this .