Waiting for answer This question has not been answered yet. You can hire a professional tutor to get the answer.

# What's the difference between isothermal process, adiabatic process, and isovolumetric process?

They essentially mean:

**isothermal**~ no change in temperature**adiabatic**~ no heat flow involved**isovolumetric**~ no change in volume

These are generally used as **assumptions** to simplify an experiment, or simply to put a situation into a more manageable problem in a chemistry course. Specifically, you should see something like this in a **Physics** course or a **Physical Chemistry** course (among others, if applicable).

I've written out some examples of what you can figure out by knowing that the situation is assumed to be such that these terms hold true.

First, some definitions:

- ##DeltaU## is the internal energy of a system.
- ##DeltaH## is the of a system.
- ##q_"rev"## is the reversible/most efficient heat flow that can occur.
- ##w_"rev"## is the reversible/most efficient work that can be performed or that something else can perform upon you.

And the following are some equations we'll end up using (Physical Chemistry: A Molecular Approach, McQuarrie).

Enthalpy vs. Internal Energy:

##\mathbf(DeltaH = DeltaU + Delta(PV))##

First Law of Thermodynamics:

##\mathbf(DeltaU = q + w)##

**ISOTHERMAL PROCESS**

Here, ##DeltaT = 0##.

For an ideal gas, that automatically means the change in internal energy ##color(blue)(DeltaU = 0)## and the change in enthalpy ##color(blue)(DeltaH = 0)##, because for an ideal gas, the internal energy and enthalpy are only dependent on the temperature.

By using this equation, you can determine the relationship between heat flow and work now, and it greatly simplifies the problem:

##cancel(DeltaH) = cancel(DeltaU) + Delta(PV)##

##= Delta(PV)##

##= PDeltaV + VDeltaP##

##color(blue)(w_"rev" = -PDeltaV = VDeltaP)##

Furthermore, using ##DeltaU = q + w##, the **first law of thermodynamics**:

##0 = q_"rev" + w_"rev"##

##color(blue)(q_"rev" = -w_"rev" = -VDeltaP)##

You couldn't say these were true unless it was an ideal gas at isothermal conditions! In my opinion, this is one situation that I find fairly straightforward.

**ADIABATIC PROCESS**

Here, ##color(blue)(q = 0)##, so using the first law of thermodynamics again:

##color(blue)(DeltaU) = cancel(q_"rev")^(0) + color(blue)(w_"rev" = -PDeltaV)##

Additionally, using the enthalpy equation from earlier:

##DeltaH = DeltaU + Delta(PV)##

##= w_"rev" + PDeltaV + VDeltaP##

##= -cancel(PDeltaV) + cancel(PDeltaV) + VDeltaP##

Thus, ##color(blue)(DeltaH = VDeltaP)## when a process upon an ideal gas is adiabatic.

**ISOVOLUMETRIC PROCESS**

A similar situation arises when ##DeltaV = 0##, because it means expansion/compression work ##color(blue)(w_"rev" = 0)## (see the above usages of ##w = -PDeltaV##?):

##color(blue)(DeltaU = q_V)##

where ##q_V## is (presumably reversible) heat flow at a constant volume.

However, it does not matter for enthalpy because if you recall from the adiabatic process, let us work backwards from the relation ##DeltaH = VDeltaP##. If it was **not** adiabatic, ##q ne 0##, thus:

##color(blue)(DeltaH = q_V + VDeltaP)##

which does not depend on ##DeltaV##.

**This can be a fairly challenging situation**, because you don't have any easy relationship where you can just do a simple integration of a ##dT## term, or a ##dV## term, or similar (giving e.g. ##PDeltaV##, ##VDeltaP##, etc).

Unless you know the following relationships, it might be difficult to figure this out in full.

##color(blue)(DeltaH) = int_(T_1)^(T_2) C_pdT##

##= color(blue)(C_p(T_2 - T_1))##

where ##C_p## is the **constant-pressure heat capacity** (doesn't have to be use in a constant-pressure situation though). For an ideal gas, it is assumed to be a constant across small temperature ranges.

From determining ##DeltaH##, you can fairly easily determine ##q##, and thus ##DeltaU##. Conveniently, you also have this relationship:

##color(blue)(DeltaU) = int_(T_1)^(T_2) C_VdT##

##= color(blue)(C_V(T_2 - T_1))##

where ##C_V##, the **constant-volume heat capacity** (doesn't have to be use in a constant-volume situation though), is based on the degrees of freedom for an ideal gas. Without going too much into this, ##C_V = 3/2 R## for a monatomic ideal gas, where ##R## is the universal gas constant, and ##C_p = C_V + nR##.

CHALLENGE: What do you imagine will be the relationships for ##DeltaU##, ##DeltaH##, ##q_"rev"##, and ##w_"rev"## for an **isobaric process**? Hint: It means constant pressure, and it is similar to the isovolumetric process.