Help l Close CHE-112-B Spring 2017 Chapter 16b t Calculating Equilibrium Concent

Question

Help l Close CHE-112-B Spring 2017 Chapter 16b t Calculating Equilibrium Concentrations previous l 3 of 14 l next t Calculating Equilibrium Concentrations 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. 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) at CO2 (g) CF4 (g), Ke 4.50 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Express your answer with the appropriate units. COF. Value Units Submit Hints My Answers Give Up Review Part Part B Consider the reaction CO(g) NH3(g) are HCONH2 (g), Ke 0.610 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? Express your answer with the appropriate units.

Explanation / Answer

2COF2(g) <==> CO2(g) + CH4 (g)

or, COF2(g) <==> (1/2)CO2(g) + (1/2)CH4 (g)

Kc = [CO2]^1/2[CH4]^1/2/[COF2]

Kc = (0.5x)^2/2-x

4.50 = 0.25x^2/2-x

or, 9-4.5x-0.25x^2 =0

or, x =1.82

equilibrium concentration of COF2 = 2-1.82 = 0.08 M

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CO(g) + Nh3(g) <==> HCONH2 (g)   Kc = 0.610

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

or, 0.610 = x/(2-3x+x^2)

or, x = 0.48

equilibrium concentration is 0.48 M

COF2 (1/2)CO2 (1/2)CF4 inital 2 0 0 change -x +0.5x +0.5x equilibrium 2-x 0.5x 0.5x

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