Concept explainers
(a)
Interpretation:
The number of air moles present initially in the tank should be determined.
Concept introduction:
The
Where, P is pressure of the gas, volume (V) occupied by the gas, temperature (T) in Kelvin, ‘n’ moles of gas and ‘R’ = Gas constant.
(b)
Interpretation:
The percentage error by neglecting the volume of the dry ice block should be determined.
Concept introduction:
The Ideal Gas Law is defined as,
Where, P is pressure of the gas, volume (V) occupied by the gas, temperature (T) in Kelvin, ‘n’ moles of gas and ‘R’ = Gas constant
(c)
Interpretation:
The final density of the gas in the tank should be determined.
Concept introduction:
The Ideal Gas Law is defined as,
Where, P is pressure of the gas, volume (V) occupied by the gas, temperature (T) in Kelvin, ‘n’ moles of gas and ‘R’ = Gas constant
(d)
Interpretation:
Explain what is happing in the tank and the variation of pressure with time.
Concept introduction:
The Ideal Gas Law is defined as,
Where, P is pressure of the gas, volume (V) occupied by the gas, temperature (T) in Kelvin, ‘n’ moles of gas and ‘R’ = Gas constant
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Chapter 5 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.arrow_forwardA 0.526 g sample of a metal, M, reacts completely with sulfuric acid according to M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g) A volume of 243 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. Calculate the molar mass of the metal.arrow_forwardPressure (A) Explain the term pressure and state its S.I. unit. (B) Explain Henry’s law. (C)A bottle of H2 has just been received by the technicians in DkIT for use in the instrumentation lab. It is a 47 litre cylinder at a pressure of 50 atmospheres. The normal working pressures is 2 bar. (i) To what volume of gas will that equate at the working pressure? (ii) For how many hours will the gas last if it used at the rate of 0.5dm3 per hour? D)You see your best friend at the bar and you walk up behind her. You accidentally startle her and she takes a step backwards. Unfortunately, she is wearing high heels and her heels come down on your foot. She weighs only 55kg but the size of her heel is 6mm by 6mm.Determine the pressure that she applies on your foot. (E) If a diver dives to a depth of 35 m what will be: (i) the pressure in Pascals due the water column? (3 marks) (ii) the pressure of the air in…arrow_forward
- A 0.210 g sample of a metal, M, reacts completely with sulfuric acid according to the reaction M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g) A volume of 219 mL of hydrogen gas is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 1.0079 bar and the temperature is 25 °C. The vapor pressure of water at 25 °C is 0.03167 bar. Calculate the molar mass of the metal.arrow_forward(a) A rigid tank contains 1.60 moles of helium, which can be treated as an ideal gas, at a pressure of 28.0 atm. While the tank and gas maintain a constant volume and temperature, a number of moles are removed from the tank, reducing the pressure to 5.00 atm. How many moles are removed? mol (b) What If? In a separate experiment beginning from the same initial conditions, including a temperature T, of 25.0°C, half the number of moles found in part (a) are withdrawn while the temperature is allowed to vary and the pressure undergoes the same change from 28.0 atm to 5.00 atm. What is the final temperature (in °C) of the gas? °Carrow_forward(a) Use the following data for NH3 (g) at T = 273 K to evaluate B2P (T). (Here Z is the compressibility factor, PV/RT). P (bar) 0.10 0.20 0.30 0.40 0.50 0.60 0.70 Note: You will need to fit this data to a least-squares line. (b) At standard temperature (273.15 K), the density of O₂ varies with pressure as indicated in the table below: P (bar) 0.25331 0.50663 0.75994 1.01325 Z-1 1.519 x 10-4 3.038 x 10-4 4.557x 10-4 6.071 x 10-4 7.583 x 10-4 9.002 x 10-4 1.0551 x 10-3 2 p(g/L) 0.356985 0.714154 1.071485 1.428962 Use this data to find the second virial coefficient, B2v, of oxygen. Note that mo2 = 31.9988 Daltons. (Hint: It will be useful to determine the molar volume from each value of p.)arrow_forward
- What is the effect of the following on the volume of 1 mol of an ideal gas?(a) The pressure is reduced by a factor of 4 (at constant T).(b) The pressure changes from 760 torr to 202 kPa, and the tem-perature changes from 37°C to 155 K.(c) The temperature changes from 305 K to 32°C, and the pres-sure changes from 2 atm to 101 kPa.arrow_forwardThe Dieterici equation of state is similar to the van der Waals equation in that they both employ gas-specific constants a and b to attempt to account for the interaction between molecules and the nonzero volume of the individual molecules of gas. However, the Dieterici equation of state has a significantly different functional form: ?(? − ?) = ??? -a ⁄ (RVT) Note that a and b are constants (n is implicitly constant as volume is expressed as molar volume). What are the following partial derivatives for the Diererici equation of state? a) (∂P/∂T)V b) (∂V/∂P)Tarrow_forwardA flue gas contains 5 mole% H 2O. Calculate the ratios(a) kmol flue gas/kmol H 2O.(b) kmol dry flue gas/kmol flue gas.(c) kmol H 2 O/kmol dry flue gas.arrow_forward
- (5) Using the data in Table 1C.3 (from the textbook), calculate the pressure that 2.500 moles of carbon dioxide confined in a volume of 1.000 L at 450 K exerts. Compare the pressure with that calculated assuming ideal-gas behavior.arrow_forwardA gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.arrow_forward3. Given the critical pressure, Pc, and the critical pressure, Tc, for CO2 are 73.75 bar and 304.13 K, respectively. (i) Assuming CO2 is an ideal gas, CALCULATE the critical volume, Vc. (ii) Assuming CO2 is a van der Waals gas, CALCULATE Vc. (iii) Assuming CO2 is a Redlich-Kwong, CALCULATE Vc. (iv) COMPARE the obtained Vc values in (i)–(iii) with that of the true Vc value; that is 0.09407 L.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
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