Part A Carbonyl fluoride, COF2 , is an important intermediate used in the produc

Question

Part A

Carbonyl fluoride, COF2 , is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction

2COF2(g)CO2(g)+CF4(g),    Kc=6.40

If only COF2 is present initially at a concentration of 2.00 M , what concentration of COF2 remains at equilibrium?

Part B

Consider the reaction:

CO(g)+NH3(g)HCONH2(g),    Kc=0.770

If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M , respectively, what will the concentration of HCONH2 be at equilibrium?

Explanation / Answer

A) 2 COF2 <=> CO2 + CF4

Inital 2 0 0

Eqm 2-2x x x

K = [CO2] [CF4] / [COF2)^2

4.60 = [x] [x] / [2 - 2x]^2

4.60 [2 - 2x]^2 = [x] [x]

4.60 [4 - 8x +4x2] = x2

18.4 - 36.8x + 18.4x2 = x2

18.4 - 36.8x + 17.4x2 = 0


x = 0.81

concentration of COF2 remains at equilibrium: 2.00 - 2x =

2.00 - 1.62 = 0.38 Molar

B)

Kc = [HCONH2] / [CO][NH3]
let X = moles/L of HCONH2 formed
[CO] = 1.00 M - X
[NH3] = 2.00 M - X
[HCONH2] = X
0.64 = X / (1.00-X)(2.00-X) = X / 2.00 - 3.00 X + X^2
0.64X^2 - 2.95X + 1.30 = 0
X = 0.48
HCONH2 = 0.48M

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