The concentration of reactants and products for a chemical reaction can be calcu

Question

The concentration of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of and/or products are known. Carbonyl fluoride, COF_2, is an important intermediate used in the production of fluoride-containing compounds. For instance, it is used to make the refrigerant carbon, CF_4 via the reaction 2COF_2 (g) reversiblearrow CO_2(g) + CF_4 (g), K_c = 7.30 if only COF_2 is present initially at a concentration of 2.00 M, what concentrations of COF_2 remains at equilibrium? Express your answer with the appropriate units. Consider the reaction CO (g) + NH_3 (g) reversiblearrow HCONH_2 (g), K_c = 0.830 If a reaction vessel initially contains only CO and NH_3 at concentrations of 1.00 M and 2.00 M. respectively, what with the concentration of HCONH_2 be at equilibrium? Express your answer with the appropriate units.

Explanation / Answer

SOLUTION:

(A)

2COF2 <--------> CO2 + CF4

I 2.0M 0 0

C -x +x +x

E (2.0 - x)M   +x +x

Kc = (x)(x) / (2.0 - x)2

7.3 = x2 / (2.0 - x)2

7.3 (4 + x2 - 4x)) = x2

29.2 + 7.3x2 - 29.2x =  x2

6.3x2 -  29.2x + 29.2 = 0 This is a quadratic equation solving it we can get th value of x as:

x = 1.46

Therefore concentration of CPF2 at equilibrium = 2.00 - 1.46 = 0.54M

(B)

CO + NH3 <-------> HCONH2

Let the concentration of HCONH2 at equilibrium is xM, Then concentration od CO and NH3 will be (1.0 -x) and

(2.0 -x) respectively

Kc = 0.830 = x / (1.0 -x)(2.0 -x)

0.830 = x / 2 -x -2x +x2

0.830 = x / 2 - 3x +x2

0.830 (2 - 3x +x2) = x

1.66 -2.49x + 0.83x2 = x

0.83x2 -3.49x + 1.66 = 0

Or x = 0.547M = 0.55M

Hence concentration of HCONH2 = 0.55M

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