Question

Solution:

Boiling point of water = 100 °C at 760 mm Hg pressure.

>> The decrease in pressure is 19.8 mm Hg for 1000 ft of elevation.

Thus, for 1.25 x 10^4 ft = 12500 ft, the decrease in pressure will be = 19.8 mm Hg x (12500 ft / 1000 ft) = 247.5 mm Hg

Thus,

The decrease in the boiling point of water

= 0.05 °C x 247.5 mm Hg = 12.4 °C

Hence,

Boiling point of water = 100 °C - 12.4 °C = 87.6 °C

#### Earn Coins

Coins can be redeemed for fabulous gifts.

Similar Homework Help Questions
• ### II Revi Part A The vapor pressure of a substance describes how readily molecules at the...

II Revi Part A 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 the atmospheric pressure exerted on the surface of the liquid. Since the atmospheric pressure at higher elevations is lower than at sea level, the boiling point of water decreases as the elevation increases. The atmospheric pressure at sea level...

• ### Boiling Point vs. Atomspheric Pressure The boiling point of water depends on atmospheric pressure. At high...

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....

• ### 1. The normal (at 760 mmHg, or 1 atm) boiling point of water is 100°C. What...

1. The normal (at 760 mmHg, or 1 atm) boiling point of water is 100°C. What mass of glucose (C6H202) would you have to dissolve in 1000 g of water to decrease the vapor pressure at 100°C by 1%? Assume that water follows Raoult's law. M(H2O) = 18.02 g/mol, M(C6H1206) = 180.2 g/mol. (10 pts) 2. What is the normal boiling point of such a solution? Assume ideal behavior. The ebullioscopic (boiling-point elevation) constant of water is Kp = 0.512...

• ### Question 3 5 pts What is the boiling point (°C) of water if the atmospheric pressure...

Question 3 5 pts What is the boiling point (°C) of water if the atmospheric pressure is 630 mmHg? atmospheric pressure)(0.037 Boiling point correction = (760 mmHg °C/mmHg) & True boiling point = 100 °C boiling point correction 4.8 O 95.2 87.3 96.4

• ### B. Boiling Point of Unknown Organic Liquid 4. Calculate the boiling point of you unknown liquid...

B. Boiling Point of Unknown Organic Liquid 4. Calculate the boiling point of you unknown liquid at 1 atm from the observed boiling point in the lab. Atmospheric pressure: 765.m g Boiling Point at 1 atm: Show your calculations below: B. Boiling Point of Unknown Organic Liquid: Unknown Observed Boiling Point Number (°C) Atmospheric Pressure (mm Hg) 765.8 mmHg 8100

• ### At sea level, water boils at 100 °C, and the absolute atmospheric pressure is 101 kPa....

At sea level, water boils at 100 °C, and the absolute atmospheric pressure is 101 kPa. As the atmospheric pressure above water decreases, the temperature required for boiling also decreases, at a rate of 3.1 kPa per "C. For the system shown below: a. What is the absolute atmospheric pressure at an elevation of 4100 m, assuming a constant unit weight of air of 11.80 N/m3? b. What will be the boiling temperature for water at this elevation? Elev. =...

• ### What is the boiling point of water at an elevation of 1.60×104 ft ? Express your...

What is the boiling point of water at an elevation of 1.60×104 ft ? Express your answer with the appropriate units using three significant figures. View Available Hint(s)

• ### Carbon disulfide, CS 2, has a heat of vaporization of 29,200 J/mol. The normal boiling point*...

Carbon disulfide, CS 2, has a heat of vaporization of 29,200 J/mol. The normal boiling point* of CS 2 is 317K What is the vapor pressure at 268K? (* BP at 760 mm Hg) Choose closest answer. 6.21 mmHg.                      26.9 mmHg. 100. mmHg                       325 mmHg. 129 mmHg.             859   mmHg. 299 mmHg. 155 mmHg.

• ### a.) Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg...

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

• ### "Vapor Pressure of Water" assignment: VAPOR PRESSURE OF WATER INTRODUCTION All liquids exist in equilibrium with...

"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...