(3) Vapor pressure of liquid ethanol is 7291 Pa at 20°C. (a) one student reports that the vapor pressure is 31741 Pa at 52°C. Another student reports it to be 31741 Pa at 502°C. Which of the results is correct? Why? (b) calculate the normal boiling temperature of ethanol (assume Patm=101,325Pa).

(3) Vapor pressure of liquid ethanol is 7291 Pa at 20°C. (a) one student reports that the vapor pressure is 31741 Pa at 52°C. Another student reports it to be 31741 Pa at 502°C. Which of the results is correct? Why? (b) calculate the normal boiling temperature of ethanol (assume Patm=101,325Pa).

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Diethyl ether, CH;OC2Hs, is a component in some hair sprays, partly because it evaporates very quickly. It has a molar volume of 103.9 cm and a vapor temperature of 18.3 torr at 25.0°C. A spray can is pressurized with 3.30 atm of gaseous propane. What is the vapor pressure of the diethyl ether in the spray can?
Given T(K)1 = 338.12 with P1 = 52.301 torr and T(K)2 = 369.52 with P2 = 141.801 torr, find the heat of vaporization (KJ/mole)?
What is the boiling point of water in a pressure cookerwith a pressure of 2.00 atm? (The enthalpy ofvaporization of water is 40.7 kJ mol–1.)(A) 101 °C (B) 121 °C (C) 141 °C (D) 200 °C
The standard enthalpy of vaporization (H°vap) of diethylether ((CH3CH2)2O) is 29.1 kJ/mol.The normal boiling point of diethylether is 34.5°C.Calculate the vapour pressure of diethylether at 19.0°C. (Units of pressure can be atm, torr, mmHg, Pa, kPa, bar, etc. -- units are always case sensitive)
For the process X(1)X(g), where X is a metal, AH°=433.4 kJ/mol and AS°-101.1 J/(K mol). What is the normal boiling point of X in °C?
Prior to the discovery that freon-12 (CF2Cl2) is harmful to the Earth’s ozone layer it was frequently used as the dispersing agent in spray cans for hair spray etc. Estimate the pressure that a can of hair spray using freon-12 has to withstand at 40 °C, the temperature of a can that has been standing in sunlight. The enthalpy of vaporization of freon-12 at its normal boiling point of −29.2 °C is 20.25 kJ mol−1; assume that this value remains constant over the temperature range of interest.
The ΔH°soln of HNO3 is –33.3 kJ/mol. 11.0 mL of 14.0 M HNO3 is dissolved in 100.0 mL of distilled water initially at 25°C. How much ice at 0°C [cP = 37.1 J/(mol ·°C), ΔH°fus = 6.01 kJ/mol] must be added to return the solution temperature to 25°C after dissolution of the acid and equilibrium with the ice is reached? The molar heat capacity is 80.8 J/(mol·°C) for the solution, and the molar heat capacity is 75.3 J/(mol·°C) for pure water.
(a) Temperature dependence of the vapor pressure of ethylene log p (mm Hg) = - 834.13 / T + 1.75 log T - 8.375 x 10-3 T + 5.3234 , which gives the temperature dependence of the molar enthalpy of vaporization derive the equation. (b) Calculate the molar enthalpy of evaporation at -103.9 oC, the normal boiling point of ethylene. Note: Use the equation that gives the temperature dependence of ΔHvap= a + bT + cT2+ ….enthalpy.
10. A piece of sodium metal reacts completely with water as follows: 2Na) + 2H2OM > 2NªOH(aq) + H2) The hydrogen gas generated is collected over water at 25.0°C. The volume of the gas is 246 mL measured at 1.00 atm. Calculate the number of grams of sodium used in the reaction. (Vapour pressure of water at 25.0°C = 0.0313 atm)
Rank the following substances in increasing boiling points (left-to-right). (a) CH4, C,H6, C;Hs, C4H10; (b) HF, HCI, HBr, and HI; (c) NH3, PH3, ASH3, and SbH3; (c) CH3OH, CH;CH;OH, CH3CI, and CH;CH;Cl; 2.
Sulfur exhibits two solid phases, rhombic and monoclinic. Use the accompanying phase diagram for sulfur given below to answer the questions that follow. (A). How many triple points are in the phase diagram? (B). What phases are in equilibrium at the topmost triple point? (C). How many phase transitions are there when rhombic sulfur at 1 atm and 80°C is heated to 500°C at constant pressure?
(a) How do the structures of these molecules account for these differences in boiling point? Provide a full account of the structures and their influence on the differences in this physical property. Name Boiling Point methane -161.6 °C methanol 64.7 °C propane -42 °C propan-1-ol 97 °C