In classical thermodynamics, if we dissipated the kinetic energy of an object as thermal energy, then we would increase the entropy. However, let's say we took 90% of some thermal energy in a reservoir, and converted it into work, and 10% of that is converted back into thermal energy after 1 minute is passed. This would mean that 81% of the thermal energy has been converted into work. If we dissipate work as heat, entropy increases. So what happens if we convert heat into work? Shouldn't the opposite occur - a decline of entropy? I think we should have a sum of changes, an entropy increase in excess of a subsequent decrease. Is this the correct view?