This document discusses the concept of dynamic equilibrium in chemistry and thermodynamics. It provides examples of dynamic equilibrium, including the transfer of carbon dioxide between the gas and liquid phases in soda until Henry's law is obeyed. Dynamic equilibrium can occur in single or multiple phase systems, such as the acid-base dissociation of acetic acid in water. The rates of the forward and backward reactions are equal at equilibrium.

1. It’s a COG thing
Balance

2. Equilibrium
Definition
State of stable conditions in which all significant
factors remain more or less constant over a period,
and there is little or no inherent tendency for
change.

3. Equilibrium in nature
DYNAMIC EQUILIBRIUM
In chemistry, a dynamic equilibrium exists once
a reversible reaction ceases to change its ratio of
reactants/products, but substances move between
the chemicals at an equal rate, meaning there is no
net change. It is a particular example of a system
in a steady state.

4. DYNAMIC EQUILIBRIUM
In thermodynamics,
a closed system is
in thermodynamic
equilibrium when reactions
occur at such rates that
the composition of the
mixture does not change
with time. Reactions do in
fact occur, sometimes
vigorously, but to such an
extent that changes in
composition cannot be
observed. Equilibrium
constants can be
expressed in terms of the

5. For
example:In a new bottle of soda the concentration of carbondioxide in
the liquid phase has a particular value. If half of the liquid is
poured out and the bottle is sealed, carbon dioxide will leave
the liquid phase at an ever-decreasing rate and the partial
pressure of carbon dioxide in the gas phase will increase until
equilibrium is reached. At that point, due to thermal motion, a
molecule of CO2 may leave the liquid phase, but within a very
short time another molecule of CO2 will pass from the gas to
the liquid, and vice versa. At equilibrium the rate of transfer
of CO2 from the gas to the liquid phase is equal to the rate
from liquid to gas.
In this case, the equilibrium concentration of CO2 in the liquid is
given by Henry's law, which states that the solubility of a gas
in a liquid is directly proportional to the partial pressure of
that gas above the liquid.

6. This relationship is written as
{display style c= kp ,}c= kp
where k is a temperature-dependent constant, p is the partial
pressure and c is the concentration of the dissolved gas in the
liquid Thus the partial pressure of CO2 in the gas has
increased until Henry's law is obeyed. The concentration of
carbon dioxide in the liquid has decreased and the drink has
lost some of its fizz.
Henry's law may be derived by setting the chemical potentials of
carbon dioxide in the two phases to be equal to each other.
Equality of chemical potential defines chemical equilibrium.
Other constants for dynamic equilibrium involving phase
changes, include partition coefficient and solubility product.
Raoult's law defines the equilibrium vapor pressure of an ideal
solutio Dynamic equilibrium can also exist in a single-phase
system. A simple example occurs with acid-base equilibrium
such as the dissociation of acetic acid, in aqueous solution.
CH3CO2H {display style right left harpoons }<-> CH3CO2− +
H+

7. At equilibrium the concentration quotient, K, the acid dissociation
constant, is constant (subject to some conditions)
{display style K_{c}=mathrm {frac {[CH_{3}CO_{2}^{-
}][H^{+}]}{[CH_{3}CO_{2}H]}} }
In this case, the forward reaction involves the liberation of
some protons from acetic acid molecules and the backward reaction
involves the formation of acetic acid molecules when an acetate ion
accepts a proton. Equilibrium is attained when the sum of chemical
potentials of the species on the left-hand side of the equilibrium
expression is equal to the sum of chemical potentials of the species
on the right-hand side. At the same time the rates of forward and
backward reactions are equal to each other.
Equilibria involving the formation of chemical complexes are also dynamic
equilibria and concentrations are governed by the stability constants
of complexes. Dynamic equilibria can also occur in the gas phase as,
for example, when nitrogen dioxide dimerizes.
2NO2 {display style right left harpoons }<-> N2O4; {displaystyle
K_{p}=mathrm {frac {[N_{2}O_{4}]}{[NO_{2}]^{2}}} }Kp=
In the gas phase, square brackets indicate partial pressure.
Alternatively, the partial pressure of a substance may be written as
P(substance).

8. Equilibrium in nature
The principle of moments
When an object is balanced (in
equilibrium) the sum of the clockwise
moments is equal to the sum of the
anticlockwise moments.
Force 1 x distance 1 from pivot = Force
2 x distance 2 from pivot
F1xd1 = F2xd2

9. When a body is in a stasis and which are its
types?
A body is in stasis when it is
motionless.
There are 3 types of stasis:
Stable
Instable
indifferent

10. Definition
o stability produced by even distribution
of weight on each side of the vertical
axis
o equipoise between contrasting,
opposing, or interacting elements
o physical equilibrium
o the ability to retain one's balance

11. The center of gravity
The centre of gravity in our
body and in any mass is the
point where the weight is
balanced.
A human's center of gravity can
change as he takes on
different positions. To locate
it, start by placing an index
finger three finger widths
below your navel to locate the
height of your center of
gravity.
Then, trace lines
around your torso at the same
level to your left and right
sides and imagine a line going

12. Balance in our Daily Life
Normal everyday activities like getting out of a chair,
walking through your home, reaching for a glass in a
cupboard, bending over to put your shoes on, driving
your car, shopping for groceries etc. depend on our
ability to control our balance. People with balance and
dizziness problems have difficulty with even the simplest
of tasks.
What is alarming is that at least half of the population
will experience balance problems sometime during their
lives, especially as they get older. In fact, poor balance
and fall related injuries account for a large percentage
of emergency room visits each year.

13. If you are an older person with a
balance problem, you’ve likely been
told that poor balance is a natural
and untreatable part of getting
older! Or worse, whether younger
or older, you’ve been told that
your “dizzy spells” are all in your
head!
If you or someone you know is
suffering from a balance disorder,
we encourage you to tour this site
to learn more about how your
balance system works and how
problems can be treated. The site
also includes information about
where to go for help, as well as an
extensive list of additional
resources and qualified clinicians.
Balance in our Daily Life

14. Balance in sports
The key to swimming fast, efficiently, and
strong is to maximize balance in the water
and minimize drag. While most of our weight
is located in our hips and lower body, this
often leads to a diagonal line in the water,
meaning that athletes literally have to drag
their body through the water. Minimizing
drag, by raising the hips closer to the
surface of the water, will not only increase a
swimmers speed, it will also increase their
efficiency by decreasing their drag.

16. https://www.sharecare.com/health/swimming/why-
balance-so-important-swimming
-NeuroCom
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