### 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 normal boiling point of a liquid is (a) the temperature at which the vapor pressure equals 1 atm. (b) the temperature at which the gas molecules have more kinetic energy than the molecules in the liquid. (c) the only temperature at which there can be equilibrium between liquid and gas. (d) the temperature at which the liquid will usually boil.
(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).
A type of alloy is a homogeneous solid mixture of metals and melts at a distinct temperature. What is this type of alloy? Give a detailed explanation of this type of alloy with a suitable example and related phase diagram.
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.
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?
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.
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 the phase diagram of carbon dioxide, the slope of the solid-liquid boundary is positive, thus the melting point decreases as pressure increases. True False