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they all look like they are

Explanation:

Only A and B are redox

Explanation:

Redox reactions are ones where elements change their oxidation states. That means any reactions that involve free elements that are also in compounds, ex: Na in a) is in both 2Na and 2NaCl are redox because their oxidation states change from 0 to whatever in the compound. This means A and B are redox reactions.

For C, (CO3) has a charge of -2, and reactants have charges C = +4, O = -2, and H = +1

The product compounds are all zero charge, so charges C = +4 and O = -2 makes CO2 charge 0 and H = +1 and O = -2 also gives H2O a zero charge. Since al elements of reactants are products do not have a change in charge, it is not redox.

Note that Oxygen is almost always at a charge of -2, that should help you with  calculations.

Similarly in d), (NO3) has charge -1, with charge N = +5, O = -2, and Pb = +2.

K tends to have charge +1 and I -1.

For d) reactants, Pb = +2 and I = -1 still gives PbI2 a zero charge. KNO3 also leaves it a zero charge.

Therefore d) also does not have any charge change in elements so it is not redox

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this