In thermodynamics, the change in internal energy (ΔU) and enthalpy (ΔH) are essential concepts for understanding heat flow during chemical reactions. When a reaction occurs at constant volume, the heat absorbed or evolved is equal to the change in internal energy (ΔU = qv). However, most chemical reactions occur at constant pressure, where the heat absorbed is equal to the enthalpy change (ΔH = qp). For an ideal gas, the relationship between ΔH and ΔU is given by the equation: ΔH = ΔU + ΔngRT; where Δng is the change in number of moles of gaseous products and reactants, R is the gas constant, and T is the temperature in Kelvin.

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CASE_STUDIESEnthalpy Change in Chemical ReactionsInternal Energy of a Thermodynamic SystemFirst Law of Thermodynamics3 sub-questions