Question

At equilibrium, the concentrations of reactants and products can
be predicted using the equilibrium constant, *K*c, which is
a mathematical expression based on the chemical equation. For
example, in the reaction

*a*A+*b*B⇌*c*C+*d*D

where *a*, *b*, *c*, and *d* are the
stoichiometric coefficients, the equilibrium constant is

*K*c=[C]*c*[D]*d*[A]*a*[B]*b*

where [A], [B], [C], and [D] are the equilibrium concentrations.
If the reaction is not at equilibrium, the quantity can still be
calculated, but it is called the reaction quotient, *Q*c,
instead of the equilibrium constant, *K*c.

*Q*c=[C]t*c*[D]t*d*[A]t*a*[B]t*b*

where each concentration is measured at some arbitrary time
*t*.

a.)A mixture initially contains A, B, and C in the following
concentrations: [A] = 0.700 *M* , [B] = 0.850 *M*,
and [C] = 0.500 *M* . The following reaction occurs and
equilibrium is established:

A+2B⇌C

At equilibrium, [A] = 0.570 *M* and [C] = 0.630
*M* . Calculate the value of the equilibrium constant,
*K*c.

Answer #1

Constructing ICE table for the reaction-

A + 2B <----> C

Initial(M): 0.700 0.850 0.500

Change: -x -2x +x

Eqlbrium: 0.700-x 0.850-2x 0.500+x

Now given,

Equilibrium concentrations,

[A]=0.570M

0.570M = 0.700M-x

x = 0.700M-0.500M = 0.130M

[C]= 0.630M

0.630M = 0.500M+x

x = 0.130M

Now keeping the value of x in [B]

[B]= 0.850-2x

[B] = 0.850-2*0.130 = 0.850M-0.260M

[B]=0.590M

Now that we know all the equilibrium concentrations-

Kc = [C]/[A][B]^{2}

= 0.630M/0.570M*(0.590M)^{2}

= 0.630M/0.19842M

Kc = 3.18

At equilibrium, the concentrations of reactants and products can
be predicted using the equilibrium constant, Kc, which is
a mathematical expression based on the chemical equation. For
example, in the reaction
aA+bB⇌cC+dD
where a, b, c, and d are the
stoichiometric coefficients, the equilibrium constant is
where [A], [B], [C], and [D] are the equilibrium concentrations.
If the reaction is not at equilibrium, the quantity can still be
calculated, but it is called the reaction quotient, Qc,
instead of the...

For chemical reactions where all reactants and products are in
the gas phase the amount of each gas in the vessel can be expressed
either as partial pressures or as concentrations. As such the
equilibrium constant for a gas phase reaction can also be expressed
in terms of concentrations or pressures. For the general
reaction,
aA(g)+bB(g)⇌cC(g)+dD(g)
Kp=(PC)c(PD)d(PA)a(PB)b
and
Kc=[C]c[D]d[A]a[B]b.
It is possible to interconvert between Kp and
Kcusing
Kp=Kc(RT)Δn
where R=0.08314 L bar mol−1 K−1 and Δn is the
difference...

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 =...

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...

Consider the following reaction and associated equilibrium
constant: aA(g)+bB(g)⇌cC(g), Kc = 5.0
a.) Find the equilibrium concentrations of A, B, and C for
a=1, b=1, and c=2. Assume that the
initial concentrations of A and B are each 1.0 M and that no
product is present at the beginning of the reaction.
Express your answer using two significant figures. Enter your
answers separated by commas.
b.) Find the equilibrium concentrations of A, B, and C for
a=1, b=1, and c=1....

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 X(g)+3Y(g)⇌2Z(g) Kp =...

Consider the following reaction and associated equilibrium
constant: aA(g)+bB(g)⇌cC(g), Kc = 3.0 Part A Find the equilibrium
concentrations of A, B, and C for a=1, b=1, and c=2. Assume that
the initial concentrations of A and B are each 1.0 M and that no
product is present at the beginning of the reaction. Express your
answer using two significant figures. Enter your answers separated
by commas. [A], [B], [C] = m M

A mixture initially contains A, B, and C in the following
concentrations: [A] = 0.700 M , [B] = 1.25 M ,
and [C] = 0.700 M . The following reaction occurs and
equilibrium is established:
A+2B⇌C
At equilibrium, [A] = 0.600 M and [C] = 0.800
M . Calculate the value of the equilibrium constant,
Kc.
Express your answer numerically.

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concentrations: [A] = 0.700 M , [B] = 1.25 M , and [C] = 0.700 M .
The following reaction occurs and equilibrium is established:
A+2B⇌C
At equilibrium, [A] = 0.500 M and [C] = 0.900 M . Calculate the
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numerically.

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A+2B⇌C
At equilibrium, [A] = 0.250 M and [C] = 0.850
M . Calculate the value of the equilibrium constant,
Kc.

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