What is the enthalpy change (ΔH) for a reaction at a constant pressure of 1.00 atm if the intern

step 1 To solve the problem, we need the following equation. Delta E equals delta H negative P delta V.

What is the enthalpy change (ΔH) for a reaction at a...

What is the enthalpy change $(\Delta H)$ for a reaction at a constant pressure of 1.00 atm if the internal energy change $(\Delta E)$ is 44.0 $\mathrm{kJ}$ and the volume increase is 14.0 $\mathrm{L}$ ?
$(1 \mathrm{L} \cdot \mathrm{atm}=101.325 \mathrm{J} .)$

Key Concepts

Energy Unit Conversions

In thermodynamics, it is often necessary to convert between different units of energy. A common conversion is between the liter-atmosphere (L·atm) unit and the joule (J), with 1 L·atm equaling approximately 101.325 J. This conversion is important when calculating energy changes in reactions where volume and pressure work are involved.

Pressure-Volume Work

Pressure-volume work is the work done when a system expands or contracts against an external pressure. Under constant pressure conditions, this work can be calculated as the product of the pressure and the change in volume (P?V). This concept is crucial for linking the internal energy change of a system to its enthalpy change.

Internal Energy

Internal energy (E) is the total energy contained within a system, encompassing all microscopic forms of energy such as kinetic and potential energies of molecules. The change in internal energy (?E) is a central concept in the first law of thermodynamics, representing the balance between the work performed by the system and the heat exchanged with its surroundings.

Enthalpy Change

Enthalpy (H) is a thermodynamic property that represents the total heat content of a system. The change in enthalpy (?H) during a reaction at constant pressure is defined as the change in internal energy (?E) plus the work done by or against the system due to pressure-volume changes. This makes it particularly useful for reactions occurring under constant atmospheric pressure, as it directly relates to the heat absorbed or released by the system.

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