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A piston filled with 0.04 mol of an idea...

A piston filled with `0.04` mol of an ideal gas expands reversibly from `50.0 mL` to `375 mL` at a constant temperature of `37.0^(@)C`. As it does so, it absorbs `208 J` of heat. The value of `q` and `w` for the process will be:
`(R=8.314J//molK)(ln 7.5=2.01)`

A

q = + 208 J, W = + 208 J

B

q = + 208 J, W = - 208 J

C

q = - 208 J, W = - 208 J

D

q = - 208 J, W = + 208 J

Text Solution

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The correct Answer is:
B
For isothermal expansion of an ideal gas `Delta U=0` Hence, from first law of thermodynamics ` Delta U=q +w` we have q = -W. As process involves adsorption of heat. I.e it is endothermic ,
q= +208 J ` therefore` W = -208 J.
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A piston filled with 0.04 mole of an ideal gas expands reversible from 50.0 mL to 375 mL at a constant temperature of 37.0^(@)C . As it does so, it absorbs 208 J of heat. The values of q and w for the process will be: (R=3.14J/molK) (in 7.5=2.01)

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