Calculating Equilibrium Concentrations The concentrations of reactants and produ

Question

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

2COF2(g)?CO2(g)+CF4(g),    Kc=7.90

Express the molar concentration numerically.

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Part B

CO(g)+NH3(g)?HCONH2(g),    Kc=0.880

Express the molar concentration numerically.

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)?CO2(g)+CF4(g),    Kc=7.90

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

Express the molar concentration numerically.

[COF2]=   M

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Part B

Consider the reaction

CO(g)+NH3(g)?HCONH2(g),    Kc=0.880

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 the molar concentration numerically.

[HCONH2]= M

Explanation / Answer

at equilibrium [CO2]= [CF4]= x and [COF2]= 2.00 - 2x

5.10 = x^2 / ( 2.00-2x)^2
solve for x

at equilibrium [HCONH2]= x , [CO]= 1.00-x and [NH3]= 2.00-x
0.660 = x / (1.00-x)(2.00-x)
solve for x

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