A piston filled with 0.04 mol of ideal gas expands reversibly from 50.0mL to 375 mLat a constant temperature of 37.0^(@)C. As it does so, itabsorbs 208J of heat. The value of q and w for the process will be : ( R= 8.314J // mol K , ln7.5 =2.01 )

A piston filled with 0.04 mol of ideal gas expands reversibly from 50.

1.	A piston filled with 0.04 mol of ideal gas expands reversibly from 50.0mL to 375 mLat a constant temperature of 37.0^(@)C. As it does so, itabsorbs 208J of heat. The value of q and w for the process will be : ( R= 8.314J // mol K , ln7.5 =2.01 )
Answer» `Q= + 208 J , w= + 208 J` `q = + 208 J , w = - 208 J` ` q = - 208 J , w= - 208 J` `q = - 208 J, w= +208 J` Solution :For isothermal EXPANSION of an ideal gas, `DeltaU = 0`. Hence,from FIRST law of thermodynamics, `DeltaU = q+w` , we have `q= -w` . As process INVOLVES adsorption of heat, i.e., it is endothermic `q= + 208 J:. W= - 208 J`