(a) Why is the change in enthalpy usually easier to measure than the change in internal energy?
(b) H is a state function, but q is not a state function. Explain.
(c) For a given process at constant pressure, \(\Delta H\) is positive. Is the process endothermic or exothermic?
Text Transcription:
\Delta H
Step 1 of 5) (a) Why is the change in enthalpy usually easier to measure than the change in internal energy(b) H is a state function, but q is not a state function. Explain.(c) For a given process at constant pressure, ΔH is positive. Is the process endothermic or exothermicIn many-electron atoms, different subshells of the same electron shell have different energies. For a given value of n, the energy of the subshells increases as the value of l increases: ns 6 np 6 and 6 nf. Orbitals within the same subshell are degenerate, meaning they have the same energy. Electrons have an intrinsic property called electron spin, which is quantized. The spin magnetic quantum number, ms, can have two possible values, +1 2 and -1 2, which can be envisioned as the two directions of an electron spinning about an axis. The Pauli exclusion principle states that no two electrons in an atom can have the same values for n, l, ml, and ms. This principle places a limit of two on the number of electrons that can occupy any one atomic orbital. These two electrons differ in their value of ms.
