The normal boiling point of mercury (Hg) is 356.7 °C. At what temperature (in °C) would the vapor pressure of mercury be 0.460 atm? (?Hvap = 58.51 kJ/mol)
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Step 1: Use the Clausius-Clapeyron equation: Ln(P2/P1) = (ΔHvap/R)(1/T1 - 1/T2) Show more…
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The normal boiling point of mercury (Hg) is 356.7 °C. At what temperature (in °C) would the vapor pressure of mercury be 0.6300 atm? (∆Hvap = 58.51 kJ/mol)
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The following data apply to the vaporization of mercury: $\Delta H_{\mathrm{vap}}=59.11 \mathrm{kJ} / \mathrm{mol} ; \Delta S_{\mathrm{vap}}=93.9 \mathrm{J} /(\mathrm{K} \cdot \mathrm{mol})$ (a) Does mercury boil at 325 °C and 1 atm pressure? (b) What is the normal boiling point of mercury?
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