Question

**Part A**

Initially, only A and B are present, each at 2.00 mol L−1. What is the final concentration of A once equilibrium is reached?

Express your answer to two significant figures and include the appropriate units.

The reversible chemical reaction

A(*a**q*)+B(*a**q*)⇌C(*a**q*)+D(*a**q*)

**Part B**

What is the final concentration of Dat equilibrium if the initial concentrations are [A] = 1.00 mol L−1 and [B] = 2.00 mol L−1 ?

Express your answer to two significant figures and include the appropriate units.

has the following equilibrium constant:

*K*=[C][D][A][B]=2.5

Answer #1

A)

A(*a**q*)+B(*a**q*)⇌C(*a**q*)+D(*a**q*)

initially:

[A] = 2

[B] = 2

[C] = 0

[D] = 0

in equilibrium

[A] = 2-x

[B] = 2-x

[C] = 0+x

[D] = 0+x

Kc = [C][D]/([A][B])

substitite

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

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

solve for x

2*sqrt(Kc) - x*sqrt(Kc) = x

(1+sqrt(Kc)) *x = 2*sqrt(Kc)

x = 2*sqrt(Kc) / (1+sqrt(Kc))

You will need the value of Kc:

then, get [A]

[A] = 2-x

[A] = 2- 2*sqrt(Kc) / (1+sqrt(Kc))

if Kc = 2.5

**[A] = 2- 2*sqrt(2.5) / (1+sqrt(2.5)) = 0.77485
M**

B)

A(*a**q*)+B(*a**q*)⇌C(*a**q*)+D(*a**q*)

initially:

[A] = 1

[B] = 2

[C] = 0

[D] = 0

in equilibrium

[A] = 1-x

[B] = 2-x

[C] = 0+x

[D] = 0+x

Kc = [C][D]/([A][B])

substitite

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

2.5 = x^2 / (1-3x+x^2)

0.4x^2 = (1-3x+x^2)

0.6x^2 -3x + 1 = 0

x = 0.359127

[A] = 1-x = 1-0.359127 = 0.6408 M

Part B
What is the final concentration of Dat equilibrium if the
initial concentrations are [A] = 1.00 mol L−1 and [B] = 2.00 mol
L−1 ?
Express your answer to two significant figures and include the
appropriate units.
The reversible chemical reaction
A(aq)+B(aq)⇌C(aq)+D(aq)
has the following equilibrium constant:
K=[C][D][A][B]=2.5
Part A
Initially, only A and B are present, each at 2.00 mol L−1. What
is the final concentration of A once equilibrium is reached?
Express your answer to two...

The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D][A][B]=7.5
Part A Initially, only A and B are present, each at 2.00 M. What
is the final concentration of A once equilibrium is reached?
Express your answer to two significant figures and include the
appropriate units.
part b What is the final concentration of D at equilibrium if
the initial concentrations are [A] = 1.00 M and [B] = 2.00
M ?
Express your answer to two significant figures...

The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D][A][B]=7.5
Part A
Initially, only A and B are present, each at 2.00 M.
What is the final concentration of A once equilibrium is
reached?
Express your answer to two significant figures and include the
appropriate units.
Part B
What is the final concentration of D at equilibrium if the
initial concentrations are[A] = 1.00 M and [B] = 2.00
M ?
Express your answer to two significant figures and...

The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D][A][B]=3.3
Part A
Initially, only A and B are present, each at 2.00 M.
What is the final concentration of A once equilibrium is
reached?
Express your answer to two significant figures and include the
appropriate units.
[A] =
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Part
Part B
What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 M and [B] = 2.00
M ?
Express...

A.) The reversible chemical reaction A+B⇌C+D has the following
equilibrium constant: Kc=[C][D][A][B]=3.9 Initially, only A and B
are present, each at 2.00 M. What is the final concentration of A
once equilibrium is reached? Express your answer to two significant
figures and include the appropriate units.
B.)What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 M and [B] = 2.00 M ? Express
your answer to two significant figures and include the...

The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D][A][B]=7.4
Part A
Initially, only A and B are present, each at 2.00 M. What is the
final concentration of A once equilibrium is reached?
Express the molar concentration numerically using two
significant figures.
Part B
What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 MM and [B] = 2.00 MM ?
Express the molar concentration numerically using two
significant figures.

The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D]/[A][B]=2.5
1. Initially, only A and B are present, each at 2.00 M.
What is the final concentration of A once equilibrium is
reached?
2.What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 M and [B] = 2.00
M ?

The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D][A][B]=3.8
Part A
Initially, only A and B are present, each at 2.00 M.
What is the final concentration of A once equilibrium is
reached?
Part B
What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 M and[B] = 2.00
M ?

The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D][A][B]=4.6
Part A
Initially, only A and B are present, each at 2.00 M.
What is the final concentration of A once equilibrium is
reached?
Part B
What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 M and [B] = 2.00
M ?

The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D][A][B]=6.7
A: initially, only A and B are present, each at 2.00 M.
What is the final concentration of A once equilibrium is
reached?
B:What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 M and [B] = 2.00
M ?
Please include all steps!

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