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 compoands. For instance, it is used to make the refrigerant carbon tetrafluoride. CF4 via the reaction If only COF-2 is present initially at a concentration of 2.00 M. what concentration of COF-2 remains at equilibrium? Consider the reaction If a reaction vessel initially contains only CO and NH_3 at concentrations of 1.00 M and 2.00 AI. respectively, what will the concentration of HCONH_2 be at equilibrium?

Explanation / Answer

The K expression

K = CO2*F2 / (COF2)^2

K = 7.7

and; in equilibrium

COF2 = 2 -2x

CO2 = 0+x

F2 = 0+x

then; substitute all

K = CO2*F2 / (COF2)^2

7.7 = x*x/(2-2x)^2

sqrt(7.7) = x/(2-2x)

2.7748 = x/(2-2x)

2-2x = 1/(2.7748)

2-2x = 0.36x

-2.36x = -2

x = 2/(2.36) = 0.8475

then

COF2 = 2-2x = 2-2*0.8475 = 0.305 M

b)

K = urea / (NH3)(CO)

K = 0.75

in equilbirium

Urea = 0+x

CO = 1-x

NH3 = 2-x

substitute in k

K = urea / (NH3)(CO)

0.75 = x /(2-x)(1-x)

1.133x = 2-3x+x^2

x^2 + (-3-1.333)x + 2 = 0

x^2 + (-4.333)x + 2 = 0

solve for x

x = 0.525195

then

since UREA = 0+x = 0.525195 M

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