A liquid has its vapor pressure measured at several temperatures. A graph of the In P vs 1/T is prepared andappears below. If the equation for the line is..y = -4699.3 k X + 2.38What is AHfor the liquid in kJ/mol?'vapYour answer should have 4 sig. figs. Do not include units on the typed answer. Just type in the number. If youwant a number in scientific notation such as 0.00034, type 3.4e-4.Inp1/TAnswer:

The temperature dependence of vapor pressure is explained by the Clausius Clapeyron equation.…

Answered: A liquid has its vapor pressure…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 13QAP

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6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of transition from white P to red P, , is . The densities of white and red phosphorus are and , respectively. At what temperature does white phosphorus become the stable phase at of pressure? Assume the formula for phosphorus is .
he following information is given for cobalt at 1atm: boiling point = 3097 °C Hvap(3097 °C) = 389 kJ/mol melting point = 1495 °C Hfus(1495 °C) = 15.5 kJ/mol specific heat solid= 0.418 J/g°C specific heat liquid = 0.686 J/g°C What is H in kJ for the process of freezing a 46.3 g sample of liquid cobalt at its normal melting point of 1495 °C. ______kJ
For the process: HXO2(g) ⇌ HXO2(l) if ΔH° is -39.04 kJ/mol and ΔS° is -111.74 J/(mol ∙ K). What is the normal boiling point of pure HXO2?
The following information is given for silver at 1atm: boiling point = 2212 °C Hvap(2212 °C) = 254 kJ/mol melting point = 961 °C Hfus(961 °C) = 12.0 kJ/mol specific heat solid= 0.238 J/g°C specific heat liquid = 0.285 J/g°C What is H in kJ for the process of freezing a 26.9 g sample of liquid silver at its normal melting point of 961 °C. ______kJ
The vapor pressure, ?,P, of a certain liquid was measured at two temperatures, ?.T. The data is shown in the table. T (K) P (kPa) 325 3.53 775 6.53 Keep the pressure units in kilopascals. If you were going to graphically determine the enthalpy of vaporizaton, Δ?vap,ΔHvap, for this liquid, what points would you plot? To avoid rounding errors, use three significant figures in the ?x‑values and four significant figures in the ?y‑values. point 1: ?=x= point 1: ?=y= point 2: ?=x= point 2: ?=y= Determine the rise, run, and slope of the line formed by these points. rise=rise= run=run= slope=slope= What is the enthalpy of vaporization of this liquid?
The following information is given for silver at 1atm: boiling point = 2212 °C Hvap(2212 °C) = 254 kJ/mol melting point = 961 °C Hfus(961 °C) = 12.0 kJ/mol specific heat solid= 0.238 J/g°C specific heat liquid = 0.285 J/g°C What is H in kJ for the process of freezing a 45.2 g sample of liquid silver at its normal melting point of 961 °C.
The normal boiling point of hexane is 69°C. Estimate 1. its enthalpy of vaporization and 2. its vapor pressure at 25°C
The following information is given for cadmium at 1atm: boiling point = 765 °C Hvap(765 °C) = 100 kJ/mol melting point = 321 °C Hfus(321 °C) = 6.11 kJ/mol specific heat solid= 0.230 J/g°C specific heat liquid = 0.264 J/g°C What is H in kJ for the process of freezing a 48.1 g sample of liquid cadmium at its normal melting point of 321 °C._______ kJ
What is Δq for the vaporization of 50.0 g of Compound A (76.03 g/mol; ΔHvap is 31.6 kJ/mol)?
At 20.0 °C, the vapor pressure of ethanol is 5.95 kPa, and at 63.5 °C, its vapor pressure is 53.3 kPa. Use this information to estimate the enthalpy of vaporization for ethanol.
Based on the calculated Δ?vap values, arrange the liquid samples in order from most ordered to least ordered. CH3OH C6H6 C4H10
A student determines the molar mass of a liquid unknown by the method used in thisexperiment. She found that the equilibrium temperature of a mixture of ice and water was1.0°C on her thermometer. When she added 12.3 g of her unknown sample to the mixture, thetemperature, after thorough stirring, fell to -4.0°C. She then poured off the solution through ascreen into a beaker. The mass of the solution was 93.4 g. Kf = 1.86°C/m What was the molality of the unknown solution? ______________ m How much unknown liquid was in the decanted solution? ______________ gHow much water was in the decanted solution? ______________ gWhat did she find to be the molar mass of the unknown liquid, assuming she made thecalculation properly?______________ g

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