QUESTION 2 Benzene freezes at 5.5°C under 1 atm. The density of benzene is 0.879 g/cm³ in liquid form and 0.891 g/cm³ in solid form. Its enthalpy of fusion is 10.59 kJ/mol. Estimate the new freezing point of benzene (°C) when pressure increase by 1300 atm. Instruction: Please round to 2 decimal places For example, 10.564 is written as 10.56. Hint: Follow the procedures of homework 4 question #4, but there are some differences: (1) You need to calculate the molar volume (unit: m³/mol) using molar mass of benzene devided by its density (pay attention to the unit which should be m3/mol), then calcualte Atrs using molar volume of liquid minus molar volume of solid (2) AtrsS can be calcualte using AfusH/T, where the unit of AfusH needs to be J/mol not kJ/mol. (3) after AT is calculated, you need to add the original freezing point to get the new freezing point.

QUESTION 2 Benzene freezes at 5.5°C under 1 atm. The density of benzene is 0.879 g/cm³ in liquid form and 0.891 g/cm³ in solid form. Its enthalpy of fusion is 10.59 kJ/mol. Estimate the new freezing point of benzene (°C) when pressure increase by 1300 atm. Instruction: Please round to 2 decimal places For example, 10.564 is written as 10.56. Hint: Follow the procedures of homework 4 question #4, but there are some differences: (1) You need to calculate the molar volume (unit: m³/mol) using molar mass of benzene devided by its density (pay attention to the unit which should be m3/mol), then calcualte Atrs using molar volume of liquid minus molar volume of solid (2) AtrsS can be calcualte using AfusH/T, where the unit of AfusH needs to be J/mol not kJ/mol. (3) after AT is calculated, you need to add the original freezing point to get the new freezing point.

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 64QAP

See similar textbooks

Similar questions

View Policies Show Attempt History Current Attempt in Progress X Incorrect. Ethanol, with AHvap = 40.5 kJ mol1, has a higher AHvap than methanol, which is 35.2 kJ mol1, due to its larger size and greater intermolecular forces. Because the AHvap for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3 °C, what would the temperature be when the vapor pressure is 8.53 atm? The temperature will be i 140 К. eTextbook and Media Hint Assistance Used Save for Later Attempts: 7 of 15 used Submit Answer !
19. The 50:50 (by mass) mix of water and ethylene glycol (antifreeze) contains 16 moles of ethylene glycol per 1 kg of water. Given than K₁ for water is 0.5 °C/m, what is the boiling point of the mixture? (A) 92 °C (B) 99.5 °C (C) 100 °C (D) 100.5 °C (E) 108 °C
Here's the Lewis structures for propane and water: HHH │││ H-C-C-C-H | B Η T I Η Η H What intermolecular forces (IMFs) would be present between a propane molecule and a water molecule? (Select all that apply) A London dispersion forces (LDFS) Dipole-dipole interactions H C Hydrogen bonding interactions с
Question 4 Calculate the change in freezing point of water, with ethalpy of fusion = 6.009 kJ/mole) and the density of ice is 0.9167 g/cc while for that liquid is 0.9999 g/cc for an increase in pressure of 1.00 atm at 273 K. Use the editor to format your answer
3. Methanol (CH;OH) has an enthalpy of fusion AHus 3.17 kJ/mol and a freezing point of -97.6 °C. Determine the AH associated with freezing 50.0 mL of methanol at -97.6 °C. (The density of methanol is 0.791 g/mL.)
The smell of fresh cut pine is due in part to the cyclic alkene pinene (136.24 g/mol) whose carbon structure is shown below. The ∆Hvap of pinene is 45.4 kJ/mol. If the vapor pressure of pinene is 101.35 kPa at 156 ºC, what is the vapor pressure at 23 ºC? Please type answer not write by hend
Consider the following liquids with similar molar masses. Predict which liquid has the highest boiling point based only on vapor pressure data. Group of answer choices pentane (vapor pressure @ 20 °C = 430 mm Hg) methyl acetate (vapor pressure @ 20 °C = 205 mm Hg) butyl alcohol (vapor pressure @ 20 °C = 6 mm Hg) propyl chloride (vapor pressure @ 20 °C = 300 mm Hg) ethyl ether (vapor pressure @ 20 °C = 450 mm Hg)
A 5.4-L closed vessel is filled with 0.46 g of liquid ethanol. This ethanol containing closed vessel is placed in the freezer and reaches the vapor pressure of 6.65 torr at -11 C. (i) Is there any liquid ethanol remained in the closed vessel when the container is removed and warmed to the temperature of 25 C? Justify your answer. (ii) How many grams of liquid ethanol remained in the vessel at 2.0 C? The enthalpy changes of vaporization, AH,vap of ethanol is 40.5 kJ/mol. The molar mass of ethanol is 46.07 g/mol.
Butane, C4H10, has a boiling point of -0.5 °C (which is 31 °F). Despite this, liquid butane can be seen sloshing about inside a typical butane lighter, even at room temperature. Why isn't the butane boiling inside the lighter at room temperature? Select all that apply. O Boiling occurs when the vapor pressure equals the surrounding pressure. O Vapor pressure decreases with increasing of temperature. O The pressure inside the lighter is higher than normal atmospheric pressure. O None of these. eTextbook and Media Save for Later Attempts: 0 of 15 used Submit Answer MacВook Air 吕0 888 DD F4 F5 F6 F7 F8 F9 F10 F2 F3 F1 @ # $ & 1 2 4 7 8 9
EXAMPLE 4-2 Vacancy Concentrations in Iron Determine the number of vacancies needed for a BCC iron crystal to have a density of 7.87 g/cm³. The lattice parameter of BCC iron is 2.866 x 10-8 cm.
What is the boiling point of a mixture composed of 55.1 g HOCH2CH3 and 399 g H2O? For H2O, Kb = 0.512 \deg C/m For H2O, Kf = 1.86 \deg C/m HOCH2CH3 = ethanol, molar mass You answer should have 3 sig figs. 46.07 g/mol
Liquid hexane (bp =69°C) is placed in a closed containerat room temperature. At first, the pressure of the vapor phase in-creases, but after a short time, it stops changing. Why?