According to the problem;
This pressure decreases by 19.8 mm Hg for every 1000- ft increase in elevation.
Total pressure drop at 1.55*10^4:
19. 8 mm Hg / 1000 ft * 1.55 x10^4 ft = 306.9 mm Hg
The boiling point of water decreases 0.05 C for every 1 mm Hg drop in atmospheric pressure.
Total temperature drop = 0.05 deg C / 1 mm Hg * 306.9 mm Hg = 15.345 deg C
Boiling point = 100 – 15.345 = 84.655 deg C
II Revi Part A The vapor pressure of a substance describes how readily molecules at the...
Part A What is the boiling point of water at an elevation of 1.25*10* ft ? Express your answer with the appropriate units using three significant figures View Available Hint(s) CHAR O ? T= Value Submit Provide Feedback <Ch 11 Assignment Vapor Pressure The vapor pressure of a substance describes how readily molecules at the surface of the substance enter the gaseous phase. At the boiling point of a liquid, the liquid's vapor pressure is equal to or greater than...
"Vapor Pressure of Water" assignment:
VAPOR PRESSURE OF WATER INTRODUCTION All liquids exist in equilibrium with the vapor state. As temperature increases, this equilibrium shifts more and more in favor of the vapor until one reaches the boiling point, at which all liquid is converted to gas. The pressure exerted by the vapor over the liquid is known as its vapor pressure and is a function of temperature. Boiling occurs at the temperature at which the vapor pressure is equal...
Question 3 (4 points) The vapor pressure of a liquid is dependent on: the temperature of the liquid and intermolecular forces of attraction in the liquid the temperature of the liquid and the surface area of the liquid only on the surface area of the liquid only the temperature of the liquid O only the forces of intermolecular attraction in the liquid Question 4 (4 points) If the atmospheric pressure over a sample of liquid is increased, the boiling point...
a.) Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg at 35°C and has a ΔHvap of 32.1 kJ/mol. b.) Determine the vapor pressure (in mm Hg) of a substance at 29°C, whose normal boiling point is 76°C and has a ΔHvap of 38.7 kJ/mol. c.) Which of the temperatures below is most likely to be the boiling point of water at 880 torr? 100°C 92°C 105°C 88°C
The vapor pressure of a liquid is the pressure exerted by its vapor when the liquid and vapor states are in equilibrium. The relationship between vapor pressure P and temperature T is expressed by the Clausius-Clapeyron equation. lnP2P1=ΔHvapR(1T1−1T2) where P1 and P2 are the vapor pressures at the absolute temperatures T1 and T2, respectively, ΔHvap is the heat of vaporization of the substance in joules per mole, and R is the ideal gas constant, which is equal to 8.3145 J/(mol⋅K)....
figure 1
Figure 2
Liquid ethanol mm P increasing P = equilibrium vapor pressure P=0 Add System comes to equilibrium ethanol Evacuated flask, pressure zero Molecules begin to vaporize, pressure increases Molecules leave and enter liquid at equal rates, pressure reaches steady-state value 34.6 °C 78.3°C 100 °C Normal boiling point Diethyl ether Vapor pressure (torr) Ethyl alcohol (ethanol) Water Ethylene glycol 100 20 40 60 80 Temperature (°C) Copyright 2009 Pearson Prentice Hall,Inc. Click on: (Figure 2) and study...
What is the normal boiling point of a substance whose vapor pressure is 67.1 mm Hg at 47°C and has a ΔHvap of 46.2 kJ/mol.
check each statement about the temperature, check each item that is
a unit of pressure, which of the following pairs of substances are
held together by hudrogen bonds, multiple choice, name the phase
16. Check each true statement about the temperature 0 K. The K stands for kilo. The K stands for Kelvin. This is a temperature that is suitable for biological processes. It is absolute zero. This temperature is the middle of the Kelvin scale. This is the coldest...
For a given pure substance, vapor pressure values were determined experimentally in equilibrium with the solid and liquid phases, at different temperatures, from which the following ratios were deduced: Solid / vapor equilibrium: ln (p / mmHg) = 17.44 - 939.7 / (T / K) Liquid / vapor balance: ln (p / mmHg) = 16.02 - 820.0 / (T / K) a) Determine the coordinates (p, T) of the triple point of the substance. b) Assuming that the enthalpy values...
Boiling Point vs. Atomspheric Pressure The boiling point of water depends on atmospheric pressure. At high altitudes, atmospheric pressure is lower, and hence water boils at a slightly lower temperature. Plot a graph by hand for the following data treating atmospheric pressure as the independent variable. Atm Press (mm of Hg) Temperature (Co) 750 752 754 756 758 760 762 764 766 768 99.63 99.70 99.78 99.85 99.93 100.00 100.07 100.15 100.22 100.29 a) Calculate the slope of the line....