Question
From the data of Table 13.4 , calculate the vibrational force constants of $\mathrm{HCl}$, HBr, and HI. Are these in the same order as the dissociation energies?
Step 1
Step 1: Recall the formula for the vibrational force constant (k) in terms of the reduced mass (μ) and the vibrational frequency (ν): k = 4π²μν² Show more…
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The separation of the lowest two vibrational levels in HBr is $0.33 \mathrm{eV}$. Find the force constant $k$ of $\mathrm{HBr}$. (Treat the bromine atom as fixed.)
Molecules
Excited States of Molecules
(1) Given that the spacing between vibrational energy levels of the HCl molecule is 0.36 eV, calculate the effective force constant. (2) Find the classical temperature associated with this difference between vibrational energy levels in HCl.
Bond dissociation energies of HF, HCl, HBr follows the order $\ldots \ldots .$ (a) $\mathrm{HBr}>\mathrm{HCl}>\mathrm{HF}$ (b) $\mathrm{HCl}>\mathrm{HBr}>\mathrm{HF}$ (c) $\mathrm{HF}>\mathrm{HBr}>\mathrm{HCl}$ (d) $\mathrm{HF}>\mathrm{HCl}>\mathrm{HBr}$
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