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**PLEASE ANSWER ALL SUB-QUESTIONS AND EXPLAIN STEP BY STEP.
THANK YOU!**
QUESTION 6 One mole of...
**PLEASE ANSWER ALL SUB-QUESTIONS AND EXPLAIN STEP BY STEP. THANK YOU!** QUESTION 6 One mole of an ideal gas is compres...
**PLEASE ANSWER ALL SUB-QUESTIONS AND EXPLAIN STEP BY STEP.
THANK YOU!**
QUESTION 6 One mole of an ideal gas is compressed isothermally but irreversibly at 130 oC from 2.5 bar to 6.5 bar in a piston/cylinder device. The work required is 30 % greater than the work of reversible, isothermal compression. The heat transferred from the gas during compression flows to a heat reservoir at 25 °C. Calculate the entropy changes of the gas, the heat reservoir, and AStotal
QUESTION...
2. One mole of an ideal gas, CP - (7/2)R and CV - (5/2)R, is compressed...
2. One mole of an ideal gas, CP - (7/2)R and CV - (5/2)R, is compressed adiabatically in a piston/cylinder device from 2 bar and 25°C to 7 bar. The process is irreversible and requires 35% more work than a reversible, adiabatic compression from the same initial state to the same final pressure. What is the entropy change of the gas?
Two mole of ideal gas, is compressed adiabatically in a piston/cylinder device from 2 bar and...
Two mole of ideal gas, is compressed adiabatically in a piston/cylinder device from 2 bar and 25oC to 7 bar. The process is irreversible and requires 25% more work than a reversible, adiabatic compression from the same initial state to the same final pressure. What is the entropy change of the gas? Assume Cv=(5/2)R in this calculation.
One mole of an ideal monoatomic gas is initially at 300 K and 5 bar of...
One mole of an ideal monoatomic gas is initially at 300 K and 5 bar of pressure inside a cylinder with a frictionless piston. a) The cylinder is kept in a heat bath and the gas is allowed to expand under 1 bar of external pressure. Calculate the work and heat associated with this process. b) Calculate the change in enthalpy for isothermal expansion at constant pressure. c) Alternatively, the gas is allowed to expand isothermally under near-equilibrium conditions. Calculate...
One hundred cubic meters of carbon dioxide initially at 150 degrees Celsius and 50 bar is...
One hundred cubic meters of carbon dioxide initially at 150 degrees Celsius and 50 bar is to be isothermally compressed in a frictionless piston-and-cylinder device to a final pressure of 300 bar. Assume that this is a reversible process. a.) Use the ideal gas equation of state to calculate: i. The volume of the compressed gas ii. The work done to compress the gas iii. The heat flow on compression b.) Use the van der Waals equation of state to...
3 1. One mole of an ideal gas expands isothermally at T = 20°C from 1.2...
3 1. One mole of an ideal gas expands isothermally at T = 20°C from 1.2 m² to 1.8 m². The gas constant is given by R= 8.314 J/mol K). (a) Calculate the work done by the gas during the isothermal expansion. W= (b) Calculate the heat transfered during the expansion Q= (c) What is the change in entropy of the gas? AS аук (c) What is the entropy change of the thermal reservoir? AS reservar JK (d) What is...
One mole of a gas at a temperature of 25 degree C and a pressure of...
One mole of a gas at a temperature of 25 degree C and a pressure of 1 bar (the initial state)is to be heated and compressed in a frictionless piston and cylinder to 300 degree C and 10 bar (the final state). a) Sketch the PV diagram and (b) compute the internal energy change, the entropy change and the heat and work required along each of the following paths: Path A: Isothermal compression to 10 bar, and then isobaric heating...
I. (30 pts.) One mole of an ideal gas with constant heat capacities and ? 5/3...
I. (30 pts.) One mole of an ideal gas with constant heat capacities and ? 5/3 is compressed adiabatically in a piston-cylinder device from T1-300 K, pi = 1 bar to p2 = 10 bar at a constant external pressure Pext"- P2 -10 bar. Calculate the final temperature, T2, and W, Q. AU, AH for this process. 2. (20 pts.) Repeat problem 1 for an adiabatic and reversible compression. 3. (20 pts.) A rigid, insulated tank is divided into two...
Question 2 One mole of an ideal gas, initially at 30 C and 1 bar is...
Question 2 One mole of an ideal gas, initially at 30 C and 1 bar is changed to 130 °C and 10 bar by using two different mechanically reversible processes: 2.1 The gas is first heated at constant pressure until its temperature is 130 °C and then compressed isothermally to 10 bar. 2.2 The gas is first compressed isothermally to 10 bar and then heated at constant pressure to 13°C Calculate Q, W, AU, and AH for each case. Take...
4. The pressure-volume diagram below shows a special reversible cycle called the Carnot cycle A mole...
4. The pressure-volume diagram below shows a special reversible cycle called the Carnot cycle A mole of an ideal gas starts off in state 1 in contact with a large thermal reservoir at temperature Th. The gas then undergoes an isothermal expansion from Vi to V2. Upon reaching state 2, the gas container is removed from contact with the thermal reservoir and covered with thermal insulation. Next the gas is allowed to expand adiabatically from V2to Vs. Because the expansion...
**PLEASE ANSWER ALL SUB-QUESTIONS AND EXPLAIN STEP BY STEP.
THANK YOU!**
QUESTION 6 One mole of an ideal gas is compressed isothermally but irreversibly at 130 oC from 2.5 bar to 6.5 bar in a piston/cylinder device. The work required is 30 % greater than the work of reversible, isothermal compression. The heat transferred from the gas during compression flows to a heat reservoir at 25 °C. Calculate the entropy changes of the gas, the heat reservoir, and AStotal
QUESTION...
2. One mole of an ideal gas, CP - (7/2)R and CV - (5/2)R, is compressed adiabatically in a piston/cylinder device from 2 bar and 25°C to 7 bar. The process is irreversible and requires 35% more work than a reversible, adiabatic compression from the same initial state to the same final pressure. What is the entropy change of the gas?
3 1. One mole of an ideal gas expands isothermally at T = 20°C from 1.2 m² to 1.8 m². The gas constant is given by R= 8.314 J/mol K). (a) Calculate the work done by the gas during the isothermal expansion. W= (b) Calculate the heat transfered during the expansion Q= (c) What is the change in entropy of the gas? AS аук (c) What is the entropy change of the thermal reservoir? AS reservar JK (d) What is...
One mole of a gas at a temperature of 25 degree C and a pressure of 1 bar (the initial state)is to be heated and compressed in a frictionless piston and cylinder to 300 degree C and 10 bar (the final state). a) Sketch the PV diagram and (b) compute the internal energy change, the entropy change and the heat and work required along each of the following paths: Path A: Isothermal compression to 10 bar, and then isobaric heating...
I. (30 pts.) One mole of an ideal gas with constant heat capacities and ? 5/3 is compressed adiabatically in a piston-cylinder device from T1-300 K, pi = 1 bar to p2 = 10 bar at a constant external pressure Pext"- P2 -10 bar. Calculate the final temperature, T2, and W, Q. AU, AH for this process. 2. (20 pts.) Repeat problem 1 for an adiabatic and reversible compression. 3. (20 pts.) A rigid, insulated tank is divided into two...
Question 2 One mole of an ideal gas, initially at 30 C and 1 bar is changed to 130 °C and 10 bar by using two different mechanically reversible processes: 2.1 The gas is first heated at constant pressure until its temperature is 130 °C and then compressed isothermally to 10 bar. 2.2 The gas is first compressed isothermally to 10 bar and then heated at constant pressure to 13°C Calculate Q, W, AU, and AH for each case. Take...
4. The pressure-volume diagram below shows a special reversible cycle called the Carnot cycle A mole of an ideal gas starts off in state 1 in contact with a large thermal reservoir at temperature Th. The gas then undergoes an isothermal expansion from Vi to V2. Upon reaching state 2, the gas container is removed from contact with the thermal reservoir and covered with thermal insulation. Next the gas is allowed to expand adiabatically from V2to Vs. Because the expansion...
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