If $w_1,w_2,w_3\text{ and }{w}_4$ for an ideal gas are magnitude of work done in isothermal, adiabatic, isobaric and isochoric reversible expansion processes, the correct order will be:

1. Isothermal Process (w₁):

In an isothermal process, the temperature of the system remains constant, and the work done by the gas is given by:

w = nRT ln (V_f / V_i)

Since the temperature is constant, the work is significant and positive when the volume increases.

2. Adiabatic Process (w₂):

In an adiabatic process, there is no heat exchange with the surroundings. The work done is related to the change in internal energy. The work done in an adiabatic expansion is less than in an isothermal process:

w = (p_f V_f - p_i V_i) / (γ - 1)

The work done is smaller than in an isothermal expansion because there is no heat input to assist in the expansion.

3. Isobaric Process (w₃):

In an isobaric process, the pressure remains constant. The work done is given by:

w = p ΔV

For the same volume change, the work done is larger than in an adiabatic process but generally less than in an isothermal process.

4. Isochoric Process (w₄):

In an isochoric process, the volume remains constant. Since work is defined as w = p ΔV, and there is no volume change, no work is done in an isochoric process. So, w₄ = 0.

Correct Order:

The correct order of work done for the processes is:

w₃ > w₁ > w₂ > w₄

Thus, the correct answer is Option d: w₃ > w₁ > w₂ > w₄.