Question

**1. Explain how energy can move spontaneously from a
system of low total energy to a system of higher total
energy.**

**2. Why is it more common to think of temperature as
being related to the rate of change of energy with respect to
entropy than it is to think of it as being related to the rate of
change of entropy with respect to energy?**

Answer #1

understand

And rate

1. To make a reaction spontaneous , Gibbs free energy need to to
move forward. Then what happen with enthalpy and entropy, how do
this terms change to make the reaction spontaneous?
2. To make a reaction non-spontaneous , Gibbs free energy need
to to move backward. Then what happen with enthalpy and entropy,
how do this terms change to make the reaction non-spontaneous?
(Use this equations to explain your answers:
S =KlnW
dG =dH -TdS
dG = G^* +...

1)
What chemicals are found in Ehrlich's reagent?!
2) The salting-out process occurs spontaneously. Can you
explain the reason for this spontaneity with free energy, enthalpy
and entropy concepts?!

Prove for an isothermal isobaric system, the particles can only
move from the region of higher Gibbs free energy to the region of
lower Gibss free energy,

Suppose we start out in a configuration with 6 total packets of
energy, with 4 in subsystem A and 2 in subsystem B. If one packet
of energy moves from A to B (so that we end up with 3 packets in
each subsystem), calculate (in terms of kB)
1. the change in entropy of subsystem A, ∆SA
2. the change in entropy of subsystem B, ∆SB
3. the change in entropy of the whole system, ∆SAB

Living organisms are highly structured, and therefore much lower
in entropy than the substances from which they grow. How is it
possible that these (local) entropy decreases can occur?
a) The Earth re-emits as much energy as it absorbs while keeping
the same temperature, so the change in heat is zero, making the
change in entropy of the Earth zero.
b) The entropy of one part of the universe can decrease provided
the total entropy of the universe increases. Energy...

Explain how the energy demand of a HVAC System can be reduced by
a focus on the distribution system

Explain how electrons can absorb and emit light to move among
different energy levels within an atom. Can light of any wavelength
be absorbed or emitted by atoms?

please explain why!!
1. An electron is released from rest in a region of space with a
nonzero electric field. As the electron moves, does the
electric potential energy of the system increase or
decrease? Explain.
2. An electron is released from rest in a region of space with a
nonzero electric field. As the electron moves, does the
electron move from a position of high to low electric
potential? Explain.

1) Explain why some substances move up the stationary pase in a
chromatographic experiment faster than others.
2) Describe how the rate of movement of a substance in a
chromatography experiment can be used to identify the
substance.

The equilibrium constant of a system, K, can be related
to the standard free energy change, ΔG∘, using the
following equation:
ΔG∘=−RTlnK
where T is a specified temperature in kelvins (usually
298 K) and R is equal to 8.314 J/(K⋅mol).
Under conditions other than standard state, the following
equation applies:
ΔG=ΔG∘+RTlnQ
In this equation, Q is the reaction quotient and is
defined the same manner as K except that the
concentrations or pressures used are not necessarily the
equilibrium values....

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