Question

Deduce jouler lare and calculation of dn for the expansion of ideal gases under isothermal.​

Answer 1

Answer:

Note that your assumption

ΔH=ΔU+W

(where W=pΔV is the pressure-volume work) only applies to processes under constant pressure p, since enthalpy is defined as

H=U+pV

and thus

dH=dU+d(pV)=dU+Vdp+pdV

which simplifies to

dH=dU+pdV

at constant pressure (dp=0).

However, the pressure does not remain constant during the process given in the question.

Answer 2

• In an ideal gas, all the collisions between molecules or atoms are perfectly elastic and no intermolecular force of attraction exists in an ideal gas because of the molecules of an ideal gas move so fast, and they are so far away from each other that they do not interact at all.
• In the case of real gas, they have negligible intermolecular attractive forces. Ideal gas does not exist naturally. However, gases behave most ideally at high temperature and low-pressure conditions.

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