The Dieterici equation of state for one mole of gas is p = R T e - a V ¯ R T V ¯ - b Where a and b are constants determined experimentally. For NH 3 (g), a = 10.91 atm. L 2 and b = 0.0404 L. Pressure p is to be calculated when V ¯ = 22.41 L and T = 273.15K. The variation of pressure from the pressure values predicted by ideal as law is to be calculated. Concept introduction: The ideal gas law considered the molecules of a gas as point particles with perfectly elastic collisions among them in nature. Thus, a modification of the ideal gas equation was coined by Johannes D. van der Waals in 1873 to consider size of molecules and the interaction forces among them. Berthelot modified the van der Waals equation as modified Berthelot model of state and further changes was made, and the equation was provided as Dieterici equation of state.

Question

An essential part of the experimental design process is to select appropriate dependent and independent variables. True False

Answer 1

Question

Chapter 1, Problem 1.56E

Interpretation Introduction

Interpretation:

The Dieterici equation of state for one mole of gas is p=RT e-aV¯RTV¯-b Where a and b are constants determined experimentally. For NH₃(g), a = 10.91 atm. L² and b = 0.0404 L. Pressure p is to be calculated when V¯=22.41 L and T = 273.15K. The variation of pressure from the pressure values predicted by ideal as law is to be calculated.

Concept introduction:

The ideal gas law considered the molecules of a gas as point particles with perfectly elastic collisions among them in nature. Thus, a modification of the ideal gas equation was coined by Johannes D. van der Waals in 1873 to consider size of molecules and the interaction forces among them. Berthelot modified the van der Waals equation as modified Berthelot model of state and further changes was made, and the equation was provided as Dieterici equation of state.

Expert Solution & Answer

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Students have asked these similar questions

An essential part of the experimental design process is to select appropriate dependent and independent variables. True False

10.00 g of Compound X with molecular formula C₂Hg are burned in a constant-pressure calorimeter containing 40.00 kg of water at 25 °C. The temperature of the water is observed to rise by 2.604 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

need help not sure what am doing wrong step by step please answer is 971A During the lecture, we calculated the Debye length at physiological salt concentrations and temperature, i.e. at an ionic strength of 150 mM (i.e. 0.150 mol/l) and a temperature of T=310 K. We predicted that electrostatic interactions are effectively screened beyond distances of 8.1 Å in solutions with a physiological salt concentration. What is the Debye length in a sample of distilled water with an ionic strength of 10.0 µM (i.e. 1.00 * 10-5 mol/l)? Assume room temperature, i.e. T= 298 K, and provide your answer as a numerical expression with 3 significant figures in Å (1 Å = 10-10 m).