A reactiont akes place at a constant pressure of 1.10 atm with an internal energy change (ΔE) of 71.5 kJ and a volume decrease of 13.6 L. What is the enthalpy change (ΔH) for the reaction? (1 L-atm = 101.325 J)

Internal energy (ΔE) is the total energy contained within a system, encompassing both kinetic and potential energy of the particles. In chemical reactions, changes in internal energy can result from heat transfer and work done on or by the system. Understanding ΔE is crucial for calculating other thermodynamic properties, such as enthalpy.

Enthalpy change (ΔH) is a measure of the heat content of a system at constant pressure. It reflects the energy absorbed or released during a reaction, accounting for both internal energy changes and the work done due to volume changes. The relationship between ΔH and ΔE is given by the equation ΔH = ΔE + PΔV, where P is pressure and ΔV is the change in volume.

In thermodynamics, work done by the system during a reaction can be calculated using the formula W = -PΔV, where P is the pressure and ΔV is the change in volume. A decrease in volume (ΔV < 0) indicates that the system is doing work on the surroundings, which affects the overall energy balance of the reaction. This concept is essential for accurately determining the enthalpy change.