11.4 If 42.0 kJ of heat is added to a 32.0-g sample of liquid meth-ane under 1 atm of pressure at a temperature of -170°C,what are the final state and temperature of the methaneonce the system equilibrates? Assume no heat is lost tothe surroundings. The normal boiling point of methane is-161.5 °C. The specific heats of liquid and gaseous meth-ane are 3.48 and 2.22 J/g-K, respectively. [Section 11.4P= 1.00 atm00%42.0 kJ(o32.0 g CH4AHvap 8.20 kJ/molT = -170 °C

Heat (q1) needed to raise the temperature from -170oC(103 K) to boiling point -161.5 oC (111.5 K)can…

Answered: 11.4 If 42.0 kJ of heat is added to a…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter14: Liquids And Solids

Section: Chapter Questions

Problem 22A

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Chloroform, CHCl3, a volatile liquid, was once used as an anesthetic but has been replaced by safer compounds. Chloroform boils at 61.7C and has a heat of vaporization of 31.4 kJ/mol. What is its vapor pressure at 37.2C?
Carbon tetrachloride, CCl4, was once used as a dry cleaning solvent, but is no longer used because it is carcinogenic. At 57.8 C, the vapor pressure of CCl4 is 54.0 kPa, and its enthalpy of vaporization is 33.05 kJ/mol. Use this information to estimate the normal boiling point for CC14.
The hydrogen fluoride molecule, HF, is more polar than a water molecule, H2O (for example, has a greater dipole moment), yet the molar enthalpy of vaporization for liquid hydrogen fluoride is lesser than that for water. Explain.
What is U when 1.00 mol of liquid water vaporizes at 100C? The heat of vaporization, Hvap, of water at 100C is 40.66 kJ/mol.
On a particular summer day, the temperature is 30.0C and the relative humidity is 80.0% (which means that the partial pressure of water vapor in the ambient air is 80.0% of the equilibrium vapor pressure of water). A sample of this air is placed in a 1.00-L flask, which is then closed and cooled to 5.0C. What is the mass (in grams) of water that still exists as vapor in the flask? How much liquid water (in grams) condenses out?
Dichloromethane, CH2Cl2,is widely used as a degreaser and paint stripper. Its vapor pressure is 381.0 mm Hg at 21.9C and 465.8 mm Hg at 26.90C. Estimate (a) its heat of vaporization (Hvap). (b) its normal boiling point.
Consider the following data for the vapor pressure of diethyl ether, a widely used anesthetic in the early days of surgery. Follow the instructions in Question 13 to estimate the heat of vaporization of diethyl ether.
The following data are the equilibrium vapor pressure of limonene, C10H16, at various temperatures. (Limonene is used as a scent in commercial products.) (a) Plot these data as ln P versus 1/T so that you have a graph resembling the one in Figure 11.13. (b) At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is it 650 mm Hg? (c) What is the normal boiling point of limonene? (d) Calculate the molar enthalpy of vaporization for limonene using the Clausius-Clapeyron equation.
An organic solvent with a molar mass of 56.45 g/mol have a normal boiling point of 45.0 °C and a normal freezing point of -14.0 ºC. If ΔHº of vaporization is 34.4 kJ/mol, ΔHº of fusion is 1.4 kJ/mol, specific heat capacity of the liquid is 2.88 J/mol.ºC ,specific heat capacity of the solid is 0.765 J/mol.ºC and specific heat capacity of the gas is 1.43 J/mol.ºC. Calculate the amount of heat (in kJ) released when 24.0 g of this solvent is converted from liquid at the normal boiling point to solid at the normal freezing point.
An organic solvent with a molar mass of 56.45 g/mol have a normal boiling point of 45.0 °C and a normal freezing point of -14.0 °C. If AH° of vaporization is 34.4 kJ/mol, AH° of fusion is 1.4 kJ/mol, specific heat capacity of the liquid is 2.88 J/mol.°C ,specific heat capacity of the solid is 0.765 J/mol.°C and specific heat capacity of the gas is 1.43 J/mol.°C. Calculate the amount of heat (in kJ) released when 24.0 g of this solvent is converted from liquid at the normal boiling point to solid at the normal freezing point. (Show your work)
If 42.0 kJ of heat is added to a 32.0-g sample of liquid methaneunder 1 atm of pressure at a temperature of -170 °C,what are the final state and temperature of the methaneonce the system equilibrates? Assume no heat is lost tothe surroundings. The normal boiling point of methane is-161.5 °C. The specific heats of liquid and gaseous methaneare 3.48 and 2.22 J/g-K, respectively.
A 337.2 g sample of acetone gas with a temperature of 56.0°C is converted to a liquid with a temperature of 56.0°C. How much heat is involved? Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°C

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