5 mole of an ideal gas expands isothermally and irreversibly from a pressure of 10 atm to 1 atm against a contant external pressure of 1 atm. `W_("irr")` at 300K is:
At 400K, 5 moles of an ideal gas expands isothermally and reversibly from 10dm^3 to 20 dm^3 . Calculate the work done by the gas.
At 27^@C , one mole of an ideal gas ocmpressed isothermally and reversibly from a pressure of 2 atm to 1.0 atm, Choose the correct option from the following
A quantity of 4.0 moles of an ideal gas at 20^(@)C expands isothermally against a constant pressure of 2.0 atm from 1.0 L to 10.0L. What is the entropy change of the system (in cals)?
One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1l to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R =0.082L atm mol^(-1)K^(-1)= 8.3J mol^(-1) K^(-1) ]
One mole of an ideal monoatomic gas at temperature T and volume 1L expands to 2L against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be:
A certain gas is expanded from (1L, 10atm) to (4L, 5atm) against a constant external pressure of 1 atm. If the initial temperature of gas is 300K and heat capacity for the process is 50J ""^(@)C^(-1) (use 1L atm = 100J), then
If the ideal gas given in the problem 45 expands against constant external pressure of 1 atm what is the q value?
If 1.5 L of an ideal gas at a pressure of 20 atm expands isothermally and reversibly to a final volume of 15 L the work done by the gas in L atm is
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
