Concept explainers
(a)
Interpretation:
Estimate the maximum cylinder temperature, if the gas is carbon dioxide.
Concept introduction:
The
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
The Soave-Redlich-Kwong (SRK) is defined as,
Where,
(b)
Interpretation:
Estimate the maximum cylinder temperature, if the gas is argon. Calculate the values predicted by the ideal gas equation.
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
The Soave-Redlich-Kwong (SRK) is defined as,
Where,
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Chapter 5 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- Under what conditions of temperature does a Redlich-Kwong gas behave like an ideal gas? Use the Redlich-Kwong equation of state to justify your answer.arrow_forward1. A perfect gas undergoes compression at constant temperature, which reduces its volumeby 3.08 dm3. The final pressure and volume of the gas are 6.42 bar and 5.38 dm3, respectively. Calculate the original pressure of the gas in (a) bar, (b) atm. 2. Consider an isothermal column of an ideal gas at 25oC. What must be the molar mass ofthis gas be if the pressure is 0.80 of its ground level value at (a) 10km and (b) 1km ? Please show complete solutionsarrow_forwardlook for critical parameters and calculate its molar volume using the real gas equation of states at 2 atm pressure and temperatures a.) T>Tc b.) T = Tc c.) T< TC of Carbon Dioxide. Describe the volume obtained.arrow_forward
- A fuel has the following volumetric analysis: CH4 = 68% C2H6 = 32% Assume complete combustion with 15% excess aur at 101.325 kPa and 27 degrees dry bulb temperature. What is the total moles in the products of combustion?arrow_forwardOne hundred moles of hydrogen gas at 298K are reversibly and isothermally compressed from 30 to 10 L. The van der Waals constants for hydrogen are a = 0.2461 L².atm/mole² and b = 0.02668/mol. In the pressure range of 0 to 1500 atm, the virial equation for hydrogen is PV = RT(1+6.4×10-4P), where P is in atmospheres. (a) Calculate the final pressure and fugacity if (i) Hydrogen behaves as an ideal gas (ii) Hydrogen behaves as a van der Waals gas (iii) Hydrogen behaves according to the virial equation. (b) Calculate the magnitude of the work that must be done on the system to achieve the required change in volume if hydrogen behaves according to the virial equationarrow_forwardYou have four samples of ideal gas, each of which contains the same number of moles of gas and has the same initial temperature, volume, and pressure. You compress each sample to one-half of its initial volume. Rank the four samples in order from highest to lowest value of the final pressure. (i) A monatomic gas compressed isothermally; (ii) a monatomic gas compressed adiabatically; (iii) a diatomic gas compressed isothermally; (iv) a diatomic gas compressed adiabatically.arrow_forward
- A rigid insulated tank is divided into 2 equal compartments by athin rigid partition. One of the compartments contains air, assumedto be an ideal gas at 800 kPa and 250◦C. The other compartment isunder a vacuum. The partition is suddenly broken and the air rushesinto the evacuated compartment. The tank pressure and temperatureeventually equilibrate. (a) what is the final temperature of the gas ◦C?(b) what is the final pressure, kPa?(c) how much work is done by the system, kJ/kg?(d) how much heat is transferred to the system kJ/kgarrow_forwardGas Constant R of CO2 at 825K.arrow_forwardConsider the following reaction CS2(g) + 3O2(g) → CO2(g) + 2SO2(g) A mixture containing only CS2(g) and excess O2(g) at a total pressure of 100 kPa is placed in a sealed vessel. After the reaction is completed and the vessel is cooled to the initial temperature, the total pressure in the vessel drops to 80 kPa. What is the mole fraction of CO2(g) in the final mixture?arrow_forward
- A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The pressure and volume of the gas are 5.04 bar and 4.65 dm³, respectively. Calculate the original pressure of the gas in (a) bar, (b) atm.arrow_forwardAn ideal gas confined to a container with a massless piston at the top. A massless wire is attacted to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 4.90 to 2.45L. When the external pressure is increased to 2.50 atm, the gas futher compresses from 2.45 to 1.96L In a seperate experiment with the same initial conditions of 2.50 atm was applied to the ideal gas, decreasing its volume from 4.90 to 1.96L in one step. If the final temperture was the same for both processes, what is the difference between q for the two step pocess and q for the one process in joules?arrow_forward1.5 kg of nitrogen gas is stored in a cylinder of 1 m length and a radius of 20.0 cm. The top of the cylinder is a moveable piston which exerts a pressure on the gas. The temperature of the gas is 80.0 degrees C. Consider the gas as ideal. The entire contraption is separated from the environment by a vacuum. A reduction of the external pressure to 60.0% of its original value takes place which leads to an expansion of the gas. Calculate the change of entropy and temperaturearrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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