1st law of thermodynamics

W = F delta x = P pistion A detla x = W = -P delta V

delta V = Q + W (work done on the system)

adiabatic - no heat removed or added

volume expands → positive work from the gas, negative work from piston

volume compresses → negative work from the gas, positive from piston

Work is area under the PV curve, difference in area is net work

Gas always pushes outwards, surrounding always pushing inwards

No volume change, no work done

In an isothermal process, Q = -W

In an Isobaric process, work is based on change in volume,

in an isovolumetric process, no work is none, change in energy = Q

In an Adiabatic process, any work (W) in the system is based on increase in internal energy (U), Q = 0

1) the net change in heat is = 0, which means the system is isolated, Qx = m(2c)(-1/3t) = -2/3mct Qy = mc(2/3t) = 2/3mct