5 moles of a monoatomic ideal gas are contained adiabatically at 50 atm pressure and 300...

5 moles of a monoatomic ideal gas are contained adiabatically at 50 atm pressure and 300 K. The pressure is suddenly released to 10 atm, and the undergoes an irreversible expansion during which it performs 4000 joules of work. Show to the final temperature of the gas after the irreversible expansion is greater than that which the would attain if the expansion from 50 to 10 atm had been conducted reversibly. Calculate the entropy product as a result of the irreversible expansion. The constant-volume molar heat capacity of the Gas is C_v has a volume of 1.5 R.

Expert Solution

genius_generous answered 2 months ago

If 4.71 moles of an ideal gas has a pressure of 3.55 atm, and a volume...

If 4.71 moles of an ideal gas has a pressure of 3.55 atm, and a volume of 26.09 L, what is the temperature of the sample in degrees Celsius?

Three moles of an ideal monatomic gas expand at a constant pressure of 2.40 atm ;...

Three moles of an ideal monatomic gas expand at a constant pressure of 2.40 atm ; the volume of the gas changes from 3.20×10-2 m3 to 4.50×10−2 m3 . a. Calculate the initial temperature of the gas. b. Calculate the final temperature of the gas. c. Calculate the amount of work the gas does in expanding. d. Calculate the amount of heat added to the gas. e. Calculate the change in internal energy of the gas.

Three moles of an ideal monatomic gas expand at a constant pressure of 2.10 atm ;...

Three moles of an ideal monatomic gas expand at a constant pressure of 2.10 atm ; the volume of the gas changes from 3.30×10−2 m3 to 4.50×10−2 m3 . a) Calculate the initial temperature of the gas. b) Calculate the final temperature of the gas. c) Calculate the amount of work the gas does in expanding. d) Calculate the amount of heat added to the gas. e) Calculate the change in internal energy of the gas

Ten moles of an ideal gas at 5 bar and 600 K is expanded adiabatically till...

Ten moles of an ideal gas at 5 bar and 600 K is expanded adiabatically till its pressure becomes 1/5th the initial pressure. Then its compressed at constant pressure and finally heated at constant volume to return to its initial state, calculate: (a) heat transfer (b) work transfer (c) internal energy and enthalpy change for each process, and for the entire cycle.Based on the results of internal energy change and enthalpy change, is the entire process follows the condition of...

Consider a monoatomic ideal gas of N moles in a gas cylinder eqilibrated at temperature T1...

Consider a monoatomic ideal gas of N moles in a gas cylinder eqilibrated at temperature T1 and pressure P1 by a mass placed on the piston. Upon removal of the mass , the gas reaches a new eqilibrium pressure P2 (<P1). Calculate the amount of work done by the gas on the surroundings for the following processes. ( You must express your answer in terms of the given variables.) 1. a nonquasistatic isothermal process (sudden removal of the mass) 2....

5 moles of ideal gas is initially at 300 K and 5 bar. It is compressed...

5 moles of ideal gas is initially at 300 K and 5 bar. It is compressed to 10 bar at 300 K. This change is carried out by two different reversible processes: A: heating at constant volume followed by cooling at constant pressure B: cooling at constant pressure followed by heating at constant volume Depict these processes on a PT graph. (Hand drawn on engineering sheet would suffice). Calculate ΔU, ΔH, Q, and W requirements for each path. Cv=20.78 J/mol.K...

Four moles of a monoatomic ideal gas in a cylinder at 27 degrees Celsius is expanded...

Four moles of a monoatomic ideal gas in a cylinder at 27 degrees Celsius is expanded at constant pressure equal to 1 atm until its volume is doubled. a) What is the change in internal energy? b) How much work was done by the gas in the process? c) How much heat was transferred to the gas?

3 moles of an ideal gas with 2 atoms under 308 K temperature and 5 atm...

3 moles of an ideal gas with 2 atoms under 308 K temperature and 5 atm are expanded reversible to 1 atm end pressure. Calculate w, q, ΔU, ΔH values in case of expansion of this expansion by isothermal and adiabatic way.

15 g of nitrogen gas at STP are adiabatically compressed to a pressure of 21 atm...

15 g of nitrogen gas at STP are adiabatically compressed to a pressure of 21 atm . What is the final temperature of the gas? What is the work done on the gas? What is the heat input to the gas? What is the compression ratio Vmax/Vmin?

An ideal gas with ?=1.4 occupies 3.0L at 300 K and 100kPapressure and is compressed adiabatically...

An ideal gas with ?=1.4 occupies 3.0L at 300 K and 100kPapressure and is compressed adiabatically until its volume is 2.0 L. It's then cooled at constant pressure until it reaches 300 K, then allowed to expand isothermally back to state A. Part A Find the net work done on the gas. Express your answer using two significant figures. Part B Find the minimum volume reached. Express your answer using two significant figures.

Question