A gas expends from `2 L` to `6L` against a constant pressure of `0.5` atm on absobing `200 J` of heat. Calculate the change in internal energy.
Text Solution
Verified by Experts
`Delta U = q+w` `= 200 J-0.5 atm (62-22)` `= 200 J-2 L atm` `= 200 J - 2 xx 101. 3 J ("1 L atm = 101.3 J")` `= - 2.6 J`
Topper's Solved these Questions
THERMODYNAMICS
RESONANCE|Exercise E-4|1 Videos
THERMODYNAMICS
RESONANCE|Exercise F-1|1 Videos
THERMODYNAMICS
RESONANCE|Exercise E-1|1 Videos
TEST SERIES
RESONANCE|Exercise CHEMISTRY|50 Videos
Similar Questions
Explore conceptually related problems
A gas expends from 1.5 to 6.5 L against a constant pressure of 0.5 atm and during this process the gas also absorbs 100 J of heat. The change in the internal energy of the gas is
An ideal gas absorbs 600cal of heat during expansion from 10L to 20L against the constant pressure of 2atm . Calculate the change in internal enegry.
A gas absorbs 200J of heat and expands against the external pressure of 1.5 atm from a volume of 0.5 litre to 1.0 litre. Calculate the change in internal energy.
A sample of gas contracts by 1 litre against a constant pressure of 0.1 atm while 5.13 J heat it lost to surroundings. The change in internal energy, U of the system is
Frictionless and weightless piston was fitted into a cylinder containing a gas This gas was allowed to expand from one litre to 5 litre against a constant pressure of one atmosphere in doing so, 200 J of heat was absorbed from the surrounding . The change in the internal energy of the system is :
A gas absorbs 200J heat and undergoes simultaneous expansion against a constant external pressure of 10^(5) Pa. The volume changes from 4L to 5L. The change in internal energy is
A gas expands in an insulated container against a constant external pressure of 1.5 atm from an initial volume of 1.2 L to 4.2 L. The change in internal energy (deltaU) of gas is nearly (1 L-atm = 101.3 J)
