resulting expression is the Clausius-Clapeyron equation for the variation of vapour pressure with temperature: dlnp Avap H dT = RT2 Clausius-Clapeyron equation (4B.9) Like the Clapeyron equation (which is exact), the Clausius- Clapeyron equation (which is an approximation) is important for understanding the appearance of phase diagrams, particu

resulting expression is the Clausius-Clapeyron equation for the variation of vapour pressure with temperature: dlnp Avap H dT = RT2 Clausius-Clapeyron equation (4B.9) Like the Clapeyron equation (which is exact), the Clausius- Clapeyron equation (which is an approximation) is important for understanding the appearance of phase diagrams, particu

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter6: Equilibria In Single-component Systems

Section: Chapter Questions

Problem 6.50E

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Similar questions

Explain the significance of the Clapeyron equation and of the Clausius-Clapeyron equation.
What is w when 1.83 kg of H20(1), initially at 25.0 °C, is converted into water vapour at 185 °C against a constant external pressure of 1.00 atm? Assume that the vapour behaves ideally and that the density of liquid water is 1.00 g/ml (Remember to include a+or-sign as appropriate.) Enter your answer in acceptable SI units, accurate to 3. significant figures. Use an acceptable Sl symbol for units.
A rigid tank contains water vapour at 250oC and an unknown pressure. When the tank is cooled to 195oC, the vapour starts condensing as shown in the figure. Estimate the initial pressure in the tank.
if ethanol has a vapor pressure of 0.08 bar and a molecular weight of 46 g/mol and water has a vapor pressure of 0.03 bar and a molecular weight of 18 g/mol. c) if the total pressure measured at these conditions is 0.02 bar, what can we conclude from the interaction between ethanol-water, respect to ethanol-ethanol and water-water? Justify your answer briefly.
Describe the changes that would be observed when water vapour at 1.0 bar and 400 K is cooled at constant pressure to 260 K. Suggest the appearance of a plot of temperature against time if energy is removed at a constant rate. To judge the relative slopes of the cooling curves, you need to know that the constant-pressure molar heat capacities of water vapour, liquid, and solid are approximately 4R, 9R, and 4.5R; the enthalpies of fusion and vaporization areΔfusHΘ = 6.01 kJ mol-1, and ΔvapHΘ = 40.7 kJ mol-1 at the appropriatetransition temperatures.
The pressure of the saturated vapor of benzene (vapor in equilibrium with liquid) is 101.32 kPa at 80°C and 4.81 kPa at 5.5°C, respectively. The latter pressure and temperature correspond to the triple point of benzene. Calculate the approximate molar heat of vaporization ∆Hmv of benzene (Clausius - Clapeyron equation).
The Prandtl number of common gases at 1 atm is about 1 for a very wide range of temperatures. Why is that so? Please explain.
The enthalpy of vaporization of a certain liquid is found to be 14.4 kJ mol−1 at 180 K, its normal boiling point. The molar volumes of the liquid and the vapour at the boiling point are 115 cm3 mol−1 and 14.5 dm3 mol−1, respectively. (a) Use the Clapeyron equation to estimate dp/dT at the normal boiling point. (b) If the Clausius–Clapeyron equation is used instead to estimate dp/dT, what is the percentage error in the resulting value of dp/dT?
Name two characteristic physical properties that distinguish condensed from gas phases, and one which distinguishes solid from liquid phases. Discuss the differences for each property. Name one colligative property and by an equation (label all variables) and 1-2 sentences the physical meaning. Consider a balloon. What thermodynamic system does it represent? How does this system interact with the environment? Calculate the heat capacity at constant pressure of methane for all its contribution and the total value according to the equipartition theorem. What is a more realistic value at room temperature? Why?
The Clausius- Clapeyron equation on the assumption that the enthalpy of vaporization is independent of temperature in the range of interest. (a) Theenthalpy of vaporization of water is 40.656 kJ mol-1 at its normal boiling temperature, 373 K. Assuming that the enthalpy of vaporization does not vary with temperature, calculate the vapour pressure of water at 308 K. (b) Derive an improved version of the equation on the basis that the enthalpy of vaporization has the form ΔvapH =a+ bT. (c) For water in the range298- 373 K, a= 57.373 kJ mol-1 and b = -44.801 J K-1 mol- 1. Use your improved version of the Clausius-Clapeyron equation to calculate a more reliable value for the vapour pressure of water at 308 K.
Q1a-> A sample of hydrogen (H₂) gas was collected over water at 60°C. If the total volume of gas collected was 53.9 mL and the atmospheric pressure was 1.14 bar, what mass (in g) of hydrogen gas was collected above the water? The vapour pressure of water at 60°C is 150 torr. Q1b=> What is the molar mass (in g mol-¹) of a gas which has a density of 1.91 g/L at a pressure of 0.91 bar and temperature 15.3°C? Your answer may not correspond to an actual gas. Do not try to identify the gas.
Understanding the connection between vapour pressure, boiling point, and enthalpy of vapourisation.