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n 2.34 mol of Hydrogen gas is initially at T = 322.0 K temperature and pi...
n = 4.81 mol of Hydrogen gas is initially at T = 323.0 K temperature and...
n = 4.81 mol of Hydrogen gas is initially at T = 323.0 K temperature and pi = 2.39×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 9.49×105 Pa. What is the volume of the gas at the end of the compression process? Tries 0/12 How much work did the external force perform? Tries 0/12 How much heat did the gas emit? Tries 0/12 How much entropy did the gas emit? Tries...
n = 4.04 mol of Hydrogen gas is initially at T = 370.0 K temperature and...
n = 4.04 mol of Hydrogen gas is initially at T = 370.0 K temperature and pi = 2.65×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 7.11×105 Pa. What is the volume of the gas at the end of the compression process? How much work did the external force perform? How much heat did the gas emit? How much entropy did the gas emit? What would be the temperature of the...
n = 3.36 mol of Hydrogen gas is initially at T = 348 K temperature and...
n = 3.36 mol of Hydrogen gas is initially at T = 348 K temperature and pi = 2.98×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 8.10×105 Pa. Volume of the gas at the end of the compression process is1.20×10-2 m^3. How much work did the external force perform? How much heat did the gas emit? How much entropy did the gas emit? What would be the temperature of the gas,...
n = 4.41 mol of Hydrogen gas is initially at T = 308 K temperature and...
n = 4.41 mol of Hydrogen gas is initially at T = 308 K temperature and pi = 1.77×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 6.63×105 Pa. A.)What is the volume of the gas at the end of the compression process? B.) How much work did the external force perform? C.)How much heat did the gas emit? D.) How much entropy did the gas emit? E.) What would be the...
n = 3.62 mol of Hydrogen gas is initially at T = 338.0 K temperature and...
n = 3.62 mol of Hydrogen gas is initially at T = 338.0 K temperature and pi = 1.77×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 8.96×105 Pa. a. What is the volume of the gas at the end of the compression process? b. How much work did the external force perform? c. How much heat did the gas emit? d. How much entropy did the gas emit? e. What would...
An ideal gas is compressed isothermally from 8.07 L to 6.35 L, at a starting pressure...
An ideal gas is compressed isothermally from 8.07 L to 6.35 L, at a starting pressure of 0.467 atm and temperature of 78.00 °C. 1. How many moles of gas are present? Tries 0/3 2. What is the final pressure (in atm) of the gas? Tries 0/3 3. If the compression is carried out reversibly and isothermally, how much work (in J) is done on the system? Tries 0/3 4. What is the heat flow in part 3? Remember that...
3. A sample of 3.0 mole of a perfect gas at 25 °C expands from 5.0...
3. A sample of 3.0 mole of a perfect gas at 25 °C expands from 5.0 L to 15.0 L. How much are the entropy changes of the system and the surroundings, and the total change in entropy in the following processes: (a) the gas expands reversibly and isothermally; (b)the gas expands isothermally but irreversibly against an external pressure of zero (Pex= 0), and (c) the gas expands adiabatically and reversibly. (20 pts)
A monatomic ideal gas that is initially at a pressure of 1.54 times 10^5 Pa and...
A monatomic ideal gas that is initially at a pressure of 1.54 times 10^5 Pa and with a volume of 8.00 times 10^-2 m^3 is compressed adiabatically to a volume of 3.90 times 10^-2 m^3. What is the final pressure? P = ______ Pa How much work is done by the gas during the compression? W = ________ J What is the ratio of the final temperature of the gas to its initial temperature?
A monatomic ideal gas is initially at volume, pressure, temperature (Vi, Pi, Ti). Consider two different...
A monatomic ideal gas is initially at volume, pressure, temperature (Vi, Pi, Ti). Consider two different paths for expansion. Path 1: The gas expands quasistatically and isothermally to (Va, Pz. T2) Path 2: First the gas expands quasistatically and adiabatically (V2, P.,T-),where you will calculate P T. Then the gas is heated quasistically at constant volume to (Va. P2 T1). a. Sketch both paths on a P-V diagram. b. Calculate the entropy change of the system along all three segments...
Consider a closed system consisting of one mole of a monoatomic ideal gas X initially at...
Consider a closed system consisting of one mole of a monoatomic ideal gas X initially at 10.0 atm, a temperature of 487.5 K, and a volume of 4.00 L (state A). From state A, the system may expand isothermally and reversibly to state B, where the pressure is 2.50 atm. The system may also expand adiabatically and reversibly to state B, where the pressure is 2.50 atm. The system may also expand adiabatically and reversibly (through an intermediate state D)...
3. A sample of 3.0 mole of a perfect gas at 25 °C expands from 5.0 L to 15.0 L. How much are the entropy changes of the system and the surroundings, and the total change in entropy in the following processes: (a) the gas expands reversibly and isothermally; (b)the gas expands isothermally but irreversibly against an external pressure of zero (Pex= 0), and (c) the gas expands adiabatically and reversibly. (20 pts)
A monatomic ideal gas that is initially at a pressure of 1.54 times 10^5 Pa and with a volume of 8.00 times 10^-2 m^3 is compressed adiabatically to a volume of 3.90 times 10^-2 m^3. What is the final pressure? P = ______ Pa How much work is done by the gas during the compression? W = ________ J What is the ratio of the final temperature of the gas to its initial temperature?
A monatomic ideal gas is initially at volume, pressure, temperature (Vi, Pi, Ti). Consider two different paths for expansion. Path 1: The gas expands quasistatically and isothermally to (Va, Pz. T2) Path 2: First the gas expands quasistatically and adiabatically (V2, P.,T-),where you will calculate P T. Then the gas is heated quasistically at constant volume to (Va. P2 T1). a. Sketch both paths on a P-V diagram. b. Calculate the entropy change of the system along all three segments...
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