At `25^(@)C`, a `0.01` mole sample of a gas is compressed in volume from `4.0 L` to `1.0 L` at constant temperature. What is work done for this process if the external pressure is `4.0` bar ?
Text Solution
AI Generated Solution
Topper's Solved these Questions
THERMODYNAMICS
RESONANCE|Exercise C-5|1 Videos
THERMODYNAMICS
RESONANCE|Exercise D-1|1 Videos
THERMODYNAMICS
RESONANCE|Exercise C-3|1 Videos
TEST SERIES
RESONANCE|Exercise CHEMISTRY|50 Videos
Similar Questions
Explore conceptually related problems
When a sample of gas expand from 4.0L to 12.0L against a constant pressure of 0.30 atm , the work involved is
One mole of an ideal gas is heated from 0^@ C to 100^@ C at a constant pressure of 1 atmosphere. Calculate the work done in the process.
Calculate the work done when 1 mol of an ideal gas is compressed reversibly from 1 bar to 4 bar at a constant temperature of 300 K
An ideal gas is allowed to expand from 1L to 10 L against a constant external pressure of 1 bar. The work doen in kJ is:
2 moles of methane gas are compressed from (1 bar,2L) to 2 bar isothermally against constant external pressure. Calculate work done in Joules.
An ideal gas is allowed to expand from 1 L to 10 L against a constant external pressure of 1 bar. Calculate the work done inkJ.