### Estimating the Normal Boiling Point of AmmoniaTo estimate the normal boiling point (in K) of ammonia, we will refer to the vapor pressure curve provided below.#### Ammonia Vapor Pressure CurveThe graph illustrates the relationship between the **vapor pressure (in torr)** and **temperature (in Kelvin, K)** for ammonia. - The **x-axis** represents the temperature, scaling from **150 K to 250 K**.- The **y-axis** measures the pressure, ranging from **0 torr to 900 torr**.The curve shows an exponential increase in vapor pressure as the temperature rises. #### Key Points on the Graph:- At lower temperatures (around 150 K), the vapor pressure is near 0 torr.- As the temperature increases to around 200 K, the vapor pressure begins to rise sharply.- At approximately 240 K, the vapor pressure nears 600 torr.#### Estimating the Boiling Point:The normal boiling point of a substance is the temperature at which its vapor pressure equals standard atmospheric pressure (1 atm, equivalent to 760 torr).From the graph:- Follow the 760 torr mark on the y-axis and trace it horizontally until it intersects with the vapor pressure curve.- Drop down from this intersection point to determine the corresponding temperature on the x-axis.#### Answer Choices:- 100 K- 205 K- 237 K- The normal boiling point cannot be determined from the diagram.Based on the graph, the intersection point for 760 torr is close to 237 K. Therefore, the normal boiling point of ammonia is approximately **237 K**.#### Conclusion:After reviewing the vapor pressure curve, we can determine that the normal boiling point of ammonia is **237 K**.

The vapor pressure curve can be used to determine the boiling point. In this process a straight…

Answered: Estimate the normal boiling point (in…

Science

Chemistry

Estimate the normal boiling point (in K) of ammonia from the vapor pressure curve below.

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

The vapor pressure of ethanol (C2H5OH) at 19 °C is 40.0torr. A 1.00-g sample of ethanol is placed in a 2.00 L containerat 19 °C. If the container is closed and the ethanolis allowed to reach equilibrium with its vapor, how manygrams of liquid ethanol remain?
Can you please help me understand how to get the answer to this question? 10. The value of (delta)Hvaporation of substance X is 65.7 kJ/mol, and its normal boiling point is 62.5 degrees Celsius. Calculate (delta)S, (delta)Ssurr, and (delta)G for th evaporation of one mole of this substance at 62.5 degrees Celsius and 1 atm.
(2) Sublimation. Figures below represent the phase diagrams for water and carbon dioxide. (a) Describe the difference in sublimation behavior under the pressure and temperature conditions prevailing on Earth. (b) How would you explain the sublimation of the polar ice caps on Mars during the Martian Summer? 217.7 METING FREZING Normal melting point Solid -Normal boiling point Liquid VAPOURISON COKDENSATION Gas 0.006 SUBLIMATION DEPOSITION 100 374.4 Temperature ("C) Pressure (atm)
Ammonia has a molar enthalpy change of vaporization equal to 24.65 kJ mol-1 at its triple point, which occurs at the temperature and pressure of 196.2 K and 49.42 torr, respectively. Calculate the normal boiling temperature of ammonia.
What is the pressure, in Pa, of water vapor in equilibrium with the liquid phase at 396.9 K?
Describe the major features of the phase diagram?
Substance X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X I have been determined: melting point enthalpy of fusion temperature (°C) 120- 110- 100- 90- 80 70- 60- You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at 20 °C is put into an evacuated flask and heated at a constant rate until 10.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. density 50+ 40 30- 20 65. °C 10.00 kJ/mol 3 2.80 g/cm³ (solid) 2.30 g/mL (liquid) 0 heat added (kJ/mol) 8 9 boiling point enthalpy of vaporization 10 heat capacity P 100. °C X 21.00 kJ/mol -1 38. J K mol (solid) 29. J.K¹ mol 48. J.K¹ mol 1 (liquid) (vapor) 2 00 ola Ar B
What feature characterizes the dynamic equilibrium between a liquid and its vapor in a closed container?
Measurements of the saturated vapor pressure of liquid SiCl4 give 0.1396 atm at 280 K and 0.4880 atm at 310 K. Calculate the normal boiling temperature of SiC14.
. The vapor pressure and enthalpy of vaporization of an unknown substance are measured to be 479.6 torr and 35.3 kJ/mol, respectively at room temperature (298.15 K). Estimate the normal boiling point of the substance at an atmospheric pressure of 760 torr.
Calculate the change in the boiling point of NH3, at the normal boiling point (239.82 K at 1 bar), per pascal change in the atmospheric pressure. The molar heat of vaporization of ammonia at the normal boiling point is 23.33 kj/mol. The molar volume of liquid ammonia is 0.02495 L/mol and the molar volume of ammonia gas at the boiling point is 19.8 L/mol
In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. The heat of vaporization of isopropanol is 44.0 kJ/mol. The vapor pressure of isopropanol at 400 torr is 67.8 °C. Calculate the normal boiling point of isopropanol. Enter your value in the first box and an appropriate unit of measure in the second box.