Question

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

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 significant figures and include the appropriate units.

Answer #1

You have

Part A

You have

From the reaction, you can see that at equilibrium C and D have the same concentration (because they have the same stoichiometric coefficient), and the concetration of B and A should be less the initial, and still the same concentration. So at equilibrium:

The K estabilshes the ration at equilibrium of all the species in the reaction. using the equation for K you can calculate X:

This yields an equation as follows:

and can be solve with the quadratic equation:

X=1.225M

so A at equilibrium is 2-1.225=0.775mol/L

Part B

As in part A, the only difference is that A and B are not equal:

Intial

Equilibrium

At equilibirum

This yields an equation as follows:

and can be solve with the quadratic equation:

X=0.792mol/L=D

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(aq)+B(aq)⇌C(aq)+D(aq)
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...

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(aq)+B(aq)⇌C(aq)+D(aq)
has the following equilibrium constant:
K=[C][D]/[A][B]=6.6
What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 mol⋅L−1 and [B] = 2.00
mol⋅L−1 ?

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]=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 ?

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