Question

Based on a *K*c value of 0.200 and the data table given,
what are the equilibrium concentrations of XY , X , and Y ,
respectively?

Express the molar concentrations numerically.

Consider mixture C, which will cause the net reaction to proceed in reverse.

Concentration
(*M*)initial:change:equilibrium:[XY]0.200+*x*0.200+*x*←net⇌[X]0.300−*x*0.300−*x*+[Y]0.300−*x*0.300−*x*

The change in concentration, *x* , is positive for the
reactants because they are produced and negative for the products
because they are consumed.

Answer #1

XY <-------------------------> X + Y

0.2 + x 0.3-x 0.3 - x

Kc = [X][Y]/[XY]

0.200 = (0.3-x)^2 / 0.2 + x

0.04 + 0.2 x = 0.09 + x^2 - 0.6 x

x^2 - 0.8 x + 0.05 = 0

x = 0.732 or x = 0.0683

equilibrium concentrations :

**[XY] = 0.268 M**

**[X] = 0.232 M**

**[Y] = 0.232 M**

The equilibrium constant, Kc, is calculated using molar
concentrations. For gaseous reactions another form of the
equilibrium constant, Kp, is calculated from partial pressures
instead of concentrations. These two equilibrium constants are
related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol),
T is the absolute temperature, and Δn is the change in the number
of moles of gas (sum moles products - sum moles reactants). For
example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which
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A+B⇌C+D
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Kc=[C][D][A][B]=7.4
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Express the molar concentration numerically using two
significant figures.
Part B
What is the final concentration of D at equilibrium if the
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Express the molar concentration numerically using two
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At equilibrium, the concentrations of reactants and products can
be predicted using the equilibrium constant, Kc, which is
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example, in the reaction
aA+bB⇌cC+dD
where a, b, c, and d are the
stoichiometric coefficients, the equilibrium constant is
Kc=[C]c[D]d[A]a[B]b
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assumptions.
Kc= 1.2
Kc= 1.8x10−2
Kc= 2.0×10−5
Express your answer using two sig figs. Enter your answers
numerically seperated by commas.

The equilibrium constant, Kc, is calculated using molar
concentrations. For gaseous reactions another form of the
equilibrium constant, Kp, is calculated from partial
pressures instead of concentrations. These two equilibrium
constants are related by the equation
Kp=Kc(RT)Δn
where R=0.08206 L⋅atm/(K⋅mol), T is the
absolute temperature, and Δn is the change in the number
of moles of gas (sum moles products - sum moles reactants). For
example, consider the reaction
N2(g)+3H2(g)⇌2NH3(g)
for which Δn=2−(1+3)=−2.
For the reaction
2A(g)+2B(g)⇌C(g)
Kc = 71.6...

The equilibrium constant, Kc, is calculated using molar
concentrations. For gaseous reactions another form of the
equilibrium constant, Kp, is calculated from partial
pressures instead of concentrations. These two equilibrium
constants are related by the equation
Kp=Kc(RT)Δn
where R=0.08206 L⋅atm/(K⋅mol), T is the
absolute temperature, and Δn is the change in the number
of moles of gas (sum moles products - sum moles reactants). For
example, consider the reaction
N2(g)+3H2(g)⇌2NH3(g)
for which Δn=2−(1+3)=−2.
A) For the reaction
3A(g)+2B(g)⇌C(g)
Kc =...

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The reaction 2CH4(g)⇌C2H2(g)+3H2(g) has an equilibrium constant of K =
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1)At equilibrium, ________.
a)the rates of the forward and reverse reactions are equal
b)the value of the equilibrium constant is 1
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e)the limiting reagent has been consumed
2)The equilibrium-constant expression depends on the ________ of
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b)
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c)
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Consider the reaction
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Trial
[A]
(M)
[B]
(M)
Rate
(M/s)
1
0.50
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2
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Express your answer to two significant figures and include the
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