To determine which metal complexes are paramagnetic and have the same number of unpaired electrons, let's analyze each one:

$[\mathrm{Co}(\mathrm{NH}_3)_6]^{3+}$:

Cobalt ion: $\mathrm{Co}^{3+}$

Electron configuration: $3d^6$

Orbital occupancy: $\mathrm{t}_{2g}^{2,2,2}$ $\mathrm{e}_{g}^{0,0}$

Magnetic property: Diamagnetic (unpaired electrons = 0)

$[\mathrm{Co}(\mathrm{C}_2 \mathrm{O}_4)_3]^{3-}$:

Cobalt ion: $\mathrm{Co}^{3+}$

Electron configuration: $3d^6$

Orbital occupancy: $\mathrm{t}_{2g}^{2,2,2}$ $\mathrm{e}_{g}^{0,0}$

Magnetic property: Diamagnetic (unpaired electrons = 0)

$[\mathrm{MnCl}_6]^{3-}$:

Manganese ion: $\mathrm{Mn}^{3+}$

Electron configuration: $3d^4$

Orbital occupancy: $\mathrm{t}_{2g}^{1,1,1}$ $\mathrm{e}_{g}^{1,0}$

Magnetic property: Paramagnetic (unpaired electrons = 4)

$[\mathrm{Mn}(\mathrm{CN})_6]^{3-}$:

Manganese ion: $\mathrm{Mn}^{3+}$

Electron configuration: $3d^4$

Orbital occupancy: $\mathrm{t}_{2g}^{2,1,1}$ $\mathrm{e}_{g}^{0,0}$

Magnetic property: Paramagnetic (unpaired electrons = 2)

$[\mathrm{CoF}_6]^{3-}$:

Cobalt ion: $\mathrm{Co}^{3+}$

Electron configuration: $3d^6$

Orbital occupancy: $\mathrm{t}_{2g}^{2,1,1}$ $\mathrm{e}_{g}^{1,1}$

Magnetic property: Paramagnetic (unpaired electrons = 4)

$[\mathrm{Fe}(\mathrm{CN})_6]^{3-}$:

Iron ion: $\mathrm{Fe}^{3+}$

Electron configuration: $3d^5$

Orbital occupancy: $\mathrm{t}_{2g}^{2,2,1}$ $\mathrm{e}_{g}^{0,0}$

Magnetic property: Paramagnetic (unpaired electrons = 1)

$[\mathrm{FeF}_6]^{3-}$:

Iron ion: $\mathrm{Fe}^{3+}$

Electron configuration: $3d^5$

Orbital occupancy: $\mathrm{t}_{2g}^{1,1,1}$ $\mathrm{e}_{g}^{1,1}$

Magnetic property: Paramagnetic (unpaired electrons = 5)

From this analysis, the paramagnetic complexes having the same number of unpaired electrons (4 unpaired electrons) are:

$[\mathrm{MnCl}_6]^{3-}$

$[\mathrm{CoF}_6]^{3-}$

These two complexes show the same paramagnetic property, each with 4 unpaired electrons.