If a process is taking place at constant temperature and pressure, delta E=0 but what about delta H?

Answer 1

#H = E + pV#

#implies dH = dE + pdV + Vdp#

Now from combined mathematical statement of the first and second laws of thermodynamics (for reversible transformations),

#TdS = dE + pdV#

Using the above relationships,

#dH = TdS + Vdp#

Integrating, one can obtain the change in #H#.

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Answer 2

If a process is taking place at constant temperature and pressure, ΔE (change in internal energy) is zero. However, ΔH (change in enthalpy) may not necessarily be zero. ΔH is the heat transferred to or from the system at constant pressure. If the process involves a chemical reaction that releases or absorbs heat, then ΔH will not be zero. It is possible for ΔH to be nonzero even when ΔE is zero, especially if the process involves expansion or compression work.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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