The concentrations of reactants and products for a chemical reaction can be calc

Question

The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of reactants and/or products are known. 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 = 8.50 initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Consider the reaction CO(g) + NH3(g) HCONH2(g), kc = 0.680 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

Hi,

A) 2 COF2 <==> CO2 + CF4
start
2.00
change
-2x. . . . . ..... .. . .+x .. .+x
at equilibrium
2.00-2x .. . . .. . ... .x. . . .x

Kc = (x)^2 / (2.00-2x)^2 = 6.40

if we take the square root of both sides of this equation

x / 2-2x = 2.53

x =5.06 - 5.06 x
6.06 x = 5.06
x = 0.835

2x = 1.67
[COF2]= 2.00 - 1.67=0.33 M

At equilibrium, 0.33 M COF2 remains

B) Kc = [HCONH2]/[CO][NH3]
In going to equilibrium, the balanced equation says that CO and NH3 will both lose x in concentration, while HCONH2 will gain x. Substitute all we know into the equation:
0.780 = x/(1.00-x)(2.00-x),
rearranges to:
0.780x

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