a. Convert the equation to one relating P(psig), V(ft³), n(lb-mole), and T(°F).b. A 30.0 mole% CO and 70.0 mole% N2 gas mixture is stored in a cylinder witha volume of 3.5 ft3 at a temperature of 85°F. The reading on a Bourdon gaugeattached to the cylinder is 500 psi. Calculate the total amount of gas (lb-mole)and the mass of CO (Ibm) in the tank.C. Approximately to what temperature (°F) would the cylinder have to be heatedto increase the gas pressure to 3000 psig, the rated safety limit of the cylinder?(The estimate would only be approximate because the ideal gas equation ofstate would not be accurate at pressures this high.) 5. The ideal-gas equation of state relates absolute pressure, P(atm); gas volume,V(liters); number of moles of gas, n(mol); and absolute temperature, T(K):PV = 0.0820nT

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Answered: a. Convert the equation to one relating…

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter17: Energy In Thermal Processes: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 58P

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A sealed cubical container 20.0 cm on a side contains a gas with three times Avogadros number of neon atoms at a temperature of 20.0C. (a) Find the internal energy of the gas. (b) Find the total translational kinetic energy of the gas. (c) Calculate the average kinetic energy per atom, (d) Use Equation 10.13 to calculate the gas pressure. (e) Calculate the gas pressure using the ideal gas law (Eq. 10.8).
15. If the specific volume of a gas is 0.800 m^3/kg, what is its specific weight? * 12.62 N/m^3 12.26 N/m^3 12.66 N/m^3 12.63 N/m^3 16. What is the mass density of a helium gas at 4 and an absolute pressure of 285 KPa. R for helium, R= 2079 J/kg-K? * 0.795 kg/m^3 0.695 Kg/m^3 0.595 Kg/m^3 0.495 Kg/m^3
36. Two moles of an ideal gas are placed in a container whose volume is8.5 3 1023 m3 . The absolute pressure of the gas is 4.5 3 105 Pa. What is the average translational kinetic energy of a molecule of the gas?
1. A sealed box with volume 2 m^3 contains an ideal gas with 2.0*10^26 particles at a temperature of 400 K. What is the pressure inside the box> a. 368 kPa b. 552 kPa c. 276 kPa d. 414 kPa 2. A sealed box with volume 1 m^3 contains an ideal gas with 2.0*10^26 particles at a temperature of 300 K. The gas is then heated isochorically to 600 K. What is the pressure inside the box? a. 5*10^29 Pa b. 1.66 MPa c. 829 kPa d. 1.38 MPa
3. Calculate for the temperature of a mol of hydrogen gas at pressure of 2.02 x 104 N/m². A mole of hydrogen gas is 2 g. Its density is 1.5 kg/m³. Assume that it follows the law of the ideal gas.
1. Suppose the amount of air in a person's lungs is 2.2 L, Calculate the number of moles of air molecules in the person’s lungs when the pressure there is atmospheric pressure. Note that the air is at 37.0°C (body temperature). 2. An expensive vacuum system can achieve a pressure as low as 1.05 × 10-7 Pa at 20°C, How many atoms are there in a cubic centimeter at this pressure and temperature?
1. A gas with a volume of 3.58×〖10〗^(-3) m^3 was placed inside a container with constant pressure of 2.58×〖10〗^4 Pa. Calculate the internal energy exerted by the gas when the volume increases four times.
2. Consider a monatomic gas in a 2-dimensional box with a rectangular area A. The velocity distribution for this gas is given by (you do not need to prove this): {-m (C +C)/ 2kT} f (C,,C,)=A e Find: A, the speed distribution, and the mean speed, C.
7. The maximum safe working pressure of a large spherical storage tank, 10 m N diameter, is 10 N/m2 (10 bar), at a temperature of 20°C. Calculate the maximum mass of helium gas that can be safely stored in the tank (molar mass of helium is 4 kg/kmol).
2. Pure helium gas is contained in a leak-proof cylinder containing a movable piston. The initial volume, pressure, and temperature of the gas are 15 L, two (2) atm, and 310 K, respectively. If the gas is rapidly compressed to 12 L and the pressure increases to 3.5 atm, what is the final temperature of the gas?
1. Let's say that we have 3.68 L of a gas was at an unknown pressure. However, at standard pressure, its volume was determined to be 9.20 L. We need to solve for the unknown pressure?
How to do

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